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Introduction to Chemistry

Bishop

Chapter 10

Chemical Calculations and Chemical Equations - all with Video Answers

Educators

Chapter Questions

04:21

Problem 1

Write balanced equations for the following reactions. You do not need to include the substances' states.
a. Hydrofluoric acid reacts with silicon dioxide to form silicon tetrafluoride and water.
b. Ammonia reacts with oxygen gas to form nitrogen monoxide and water.
c. Water solutions of nickel(II) acetate and sodium phosphate react to form solid nickel(II) phosphate and aqueous sodium acetate.
d. Phosphoric acid reacts with potassium hydroxide to form water and potassium phosphate.

Daniel Kim
Daniel Kim
Numerade Educator
04:03

Problem 2

Write complete equations, including states, for the precipitation reaction that takes place between the reactants in part (a) and the neutralization reaction that takes place in part (b).
a. $\mathrm{Ca}\left(\mathrm{NO}_3\right)_2(a q)+\mathrm{Na}_2 \mathrm{CO}_3(a q) \rightarrow$
b. $\mathrm{HNO}_3(\mathrm{aq})+\mathrm{Al}(\mathrm{OH})_3(s) \rightarrow$

David Collins
David Collins
Numerade Educator
00:32

Problem 3

How many moles of phosphorous acid, $\mathrm{H}_3 \mathrm{PO}_3$, are there in 68.785 g of phosphorous acid?

David Collins
David Collins
Numerade Educator
02:00

Problem 4

What is the mass in kilograms of 0.8459 mole of sodium sulfate?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:36

Problem 5

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
If a calculation calls for you to convert from an amount of one substance in a given chemical reaction to the corresponding amount of another substance participating in the same reaction, it is an equation _______ problem.

Carlene Jimenez
Carlene Jimenez
Numerade Educator

Problem 6

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
The coefficients in $\mathrm{a}(\mathrm{n})$ _______ provide us with information that we can use to build conversion factors that convert from an amount of one substance in a given chemical reaction to the corresponding amount of another substance participating in the same reaction.

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Problem 7

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
For some chemical reactions, chemists want to mix reactants in amounts that are as close as possible to the ratio that would lead to the complete reaction of each. This ratio is sometimes called the _______ ratio.

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Problem 8

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
$\mathrm{A}(\mathrm{n})$ _______ of one or more of the reactants will increase the likelihood that the other reactant or reactants will be used up. Thus, if one reactant is more expensive than the others, adding an excess of the _______ expensive reactants will ensure the greatest conversion possible of the one that is
_______

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Problem 9

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
Sometimes one product is more important than others are, and the amounts of reactants are chosen to _______ its production.

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Problem 10

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
Any component added in excess will _______ when the reaction is complete. If one reactant is more dangerous to handle than others are, chemists would rather not have that reactant _______ at the reaction's end.

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Problem 11

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
Because some of the reactant that was added in excess is likely to be mixed with the product, chemists would prefer that the substance in excess be a substance that is
_______ from the primary product.

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Problem 12

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
The reactant that _______ in a chemical reaction limits the amount of product that can form. This reactant is called the limiting reactant.

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Problem 13

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
The tip-off for limiting reactant problems is that you are given
_______ of reactants in a chemical reaction, and you are asked to calculate the maximum _______ that they can form.

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Problem 14

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
The theoretical yield is the maximum amount of product that could be formed from the given amounts of reactants. This is the amount of product that could be obtained if _______ of the limiting reactant were converted to product and if this product could be isolated from the other components in the product mixture without any _______ . The efficiency of a reaction can be evaluated by calculating the percent yield, the ratio of the _______ yield to the theoretical yield expressed as a percentage.

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02:43

Problem 15

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
There are many reasons why the actual yield in a reaction might be less than the theoretical yield. One key reason is that many chemical reactions are significantly
_______

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator

Problem 16

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
A reaction's yield is also affected by the occurrence of _______

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Problem 17

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
Another factor that affects the actual yield is a reaction's rate. Sometimes a reaction is so _______ that it has not reached the maximum yield by the time the product is isolated.

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Problem 18

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
Even if $100 \%$ of the limiting reactant proceeds to products, usually the product still needs to be _______ from the other components in the product mixture (excess reactants, products of side reactions, and other impurities). This process generally leads to some loss of product.

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Problem 19

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
When two solutions are mixed to start a reaction, it is more convenient to measure their $\qquad$ than their masses.

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Problem 20

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
Molarity (abbreviated M) is defined as moles of ________ per liter of ________
________

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Problem 21

Complete the following statements by writing one of these words or phrases in each
blank.
$$
\begin{array}{ll}
100 \% & \begin{array}{l}
\text { remaining } \\
\text { actual } \\
\text { reversible }
\end{array} \\
\text { amount of product } & \text { runs out first } \\
\text { balanced chemical equation } & \text { separated } \\
\text { costly } & \text { side reactions } \\
\text { easy to separate } & \text { slow } \\
\text { excess } & \text { solute } \\
\text { less } & \text { solution } \\
\text { loss } & \text { stoichiometric } \\
\text { mass } & \text { stoichiometry } \\
\text { molar mass } & \text { two or more amounts } \\
\text { optimize } & \text { volume of solution } \\
\text { remain } & \text { volumes }
\end{array}
$$
Conversion factors constructed from molarities can be used in stoichiometric calculations in very much the same way conversion factors from ________ are used. When a substance is pure, its molar mass can be used to convert back and forth between the measurable property of ________ and moles. When a substance is in solution, its molarity can be used to convert between the measurable property of ________ and moles of solute.

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00:46

Problem 22

Because the bond between fluorine atoms in $\mathrm{F}_2$ is relatively weak while the bonds between fluorine atoms and atoms of other elements are relatively strong, it is difficult to make diatomic fluorine, $\mathrm{F}_2$. One way it can be made is to run an electric current through liquid hydrogen fluoride, HF. This reaction yields hydrogen gas, $\mathrm{H}_2$, and fluorine gas, $\mathrm{F}_2$.
a. Write a complete balanced equation, including states, for this reaction.
b. Draw a picture of the reaction, using rough sketches of space-filling models in place of the coefficients and formulas in the equation. Fluorine atoms have a little more than twice the diameter of hydrogen atoms.
c. Write a conversion factor that could be used to convert between moles of HF and moles of $\mathrm{F}_2$.
d. How many moles of $\mathrm{F}_2$ form when one mole of HF reacts completely?
e. How many moles of HF react to yield 3.452 moles of $\mathrm{H}_2$ ?

Sam Limsuwannarot
Sam Limsuwannarot
Numerade Educator
03:56

Problem 23

Hydrogen gas is used for many purposes, including the hydrogenation of vegetable oils to make margarine. The most common industrial process for producing hydrogen is "steam reforming," in which methane gas, $\mathrm{CH}_4$, from natural gas reacts with water vapor to form carbon monoxide gas and hydrogen gas.
a. Write a complete balanced equation, including states, for this reaction.
b. Draw a picture of the reaction, using rough sketches of space-filling models in place of the coefficients and formulas in the equation. Draw the carbon atoms a little larger than the oxygen atoms. Both carbon and oxygen atoms have over twice the diameter of hydrogen atoms.
c. Write a conversion factor that could be used to convert between moles of methane and moles of hydrogen.
d. How many moles of hydrogen form when 4 moles of methane react completely?
e. How many moles of water vapor react to yield 174.82 moles of hydrogen?

Daniel Kim
Daniel Kim
Numerade Educator
04:27

Problem 24

The bond between nitrogen atoms in $\mathrm{N}_2$ molecules is very strong, making $\mathrm{N}_2$ very unreactive. Because of this, magnesium is one of the few metals that react with nitrogen gas directly. This reaction yields solid magnesium nitride.
a. Write a complete balanced equation, without including states, for the reaction between magnesium and nitrogen to form magnesium nitride.
b. Write a conversion factor that could be used to convert between moles of magnesium and moles of magnesium nitride.
c. How many moles of magnesium nitride form when 1.0 mole of magnesium reacts completely?
d. Write a conversion factor that could be used to convert between moles of nitrogen and moles of magnesium nitride.
e. How many moles of nitrogen react to yield 3.452 moles of magnesium nitride?

Banhishikha Sinha
Banhishikha Sinha
Numerade Educator
03:53

Problem 25

Fluorine gas is an important chemical because it is used to add fluorine atoms to many different compounds. As mentioned in Problem 22, it is difficult to make, but the following two-step process produces fairly high yields of $\mathrm{F}_2$.

$$
\begin{aligned}
& 2 \mathrm{KMnO}_4+2 \mathrm{KF}+10 \mathrm{HF}+3 \mathrm{H}_2 \mathrm{O}_2 \rightarrow 2 \mathrm{~K}_2 \mathrm{MnF}_6+8 \mathrm{H}_2 \mathrm{O}+3 \mathrm{O}_2 \\
& 2 \mathrm{~K}_2 \mathrm{MnF}_6+4 \mathrm{SbF}_5 \rightarrow 4 \mathrm{KSbF}_6+2 \mathrm{MnF}_3+\mathrm{F}_2
\end{aligned}
$$

For the second of these two reactions:
a. Write a conversion factor that could be used to convert between moles of antimony pentafluoride, $\mathrm{SbF}_5$, and moles of fluorine, $\mathrm{F}_2$.
b. How many moles of $\mathrm{F}_2$ form when 8 moles of $\mathrm{SbF}_5$ react completely?
c. What is the maximum number of moles of $\mathrm{F}_2$ that could form in the combination of 2.00 moles of $\mathrm{K}_2 \mathrm{MnF}_6$ and 5.00 moles of $\mathrm{SbF}_5$ ?
d. What is the maximum number of moles of $\mathrm{F}_2$ that could form in the combination of 2 moles of $\mathrm{K}_2 \mathrm{MnF}_6$ and 5000 moles of $\mathrm{SbF}_5$ ?
e. Write a conversion factor that could be used to convert between moles of manganese(III) fluoride, $\mathrm{MnF}_3$, and moles of $\mathrm{F}_2$.
f. How many moles of $\mathrm{F}_2$ form along with 0.802 mole of $\mathrm{MnF}_3$ ?

AK
Acadia Kopec
Numerade Educator
06:32

Problem 26

For many years, it was thought that no reaction could produce sodium perbromate, but the discovery of a reaction producing the equally elusive xenon difluoride, $\mathrm{XeF}_2$, led to the discovery of the following reaction that yields sodium perbromate.

$$
\mathrm{NaBrO}_3+\mathrm{XeF}_2+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{NaBrO}_4+2 \mathrm{HF}+\mathrm{Xe}
$$

a. Write a conversion factor that could be used to convert between moles of xenon difluoride, $\mathrm{XeF}_2$, and moles of hydrogen fluoride, HF .
b. How many moles of $\mathrm{XeF}_2$ are necessary to form 16 moles of hydrogen fluoride?
c. What is the maximum number of moles of $\mathrm{NaBrO}_4$ that could form in the combination of 2 moles of $\mathrm{NaBrO}_3$ and 3 moles of $\mathrm{XeF}_2$ ?
d. What is the maximum number of moles of $\mathrm{NaBrO}_4$ that could form in the combination of 2 moles of $\mathrm{NaBrO}_3$ and 3 million moles of $\mathrm{XeF}_2$ ?
e. Write a conversion factor that could be used to convert between moles of sodium perbromate, $\mathrm{NaBrO}_4$, and moles of hydrogen fluoride, HF .
f. How many moles of HF form along with 5.822 moles of sodium perbromate, $\mathrm{NaBrO}_4$ ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:54

Problem 27

The thiocyanate polyatomic ion, $\mathrm{SCN}^{-}$, is commonly called a pseudohalogen because it acts very much like halide ions. For example, we know that the pure halogens consist of diatomic molecules, such as $\mathrm{Cl}_2$. Thiocyanate ions form similar molecules in the following reaction:

$$
2 \mathrm{NaSCN}+2 \mathrm{H}_2 \mathrm{SO}_4+\mathrm{MnO}_2 \rightarrow(\mathrm{SCN})_2+2 \mathrm{H}_2 \mathrm{O}+\mathrm{MnSO}_4+\mathrm{Na}_2 \mathrm{SO}_4
$$

a. Write a conversion factor that could be used to convert between moles of NaSCN and moles of $(\mathrm{SCN})_2$.
b. How many moles of $(\mathrm{SCN})_2$ form when 0.50 moles of NaSCN react completely?
c. What is the maximum number of moles of $(\mathrm{SCN})_2$ that could form in the combination of 4 moles of NaSCN and 3 moles of $\mathrm{MnO}_2$ ?
d. Write a conversion factor that could be used to convert between moles of sulfuric acid, $\mathrm{H}_2 \mathrm{SO}_4$, and moles of manganese(II) sulfate, $\mathrm{MnSO}_4$.
e. What is the minimum number of moles of $\mathrm{H}_2 \mathrm{SO}_4$ that must react to form 1.7752 moles of manganese(II) sulfate?

Aadit Sharma
Aadit Sharma
Numerade Educator
01:05

Problem 28

In Chapter 3, you were told that halogen atoms generally form a single covalent bond, but there are many compounds in which halogen atoms form more than one bond. For example, bromine pentafluoride (used as an oxidizing agent in rocket propellants) has bromine atoms with five covalent bonds. Liquid bromine pentafluoride is the only product in the reaction of gaseous bromine monofluoride with fluorine gas.
a. Write a complete balanced equation, including states, for this reaction.
b. Write a conversion factor that could be used to convert between moles of fluorine and moles of bromine pentafluoride.
c. How many moles of bromine pentafluoride form when 6 moles of fluorine react completely?
d. What is the maximum number of moles of bromine pentafluoride that could form in the combination of 8 moles of bromine monofluoride with 12 moles of fluorine?
e. Write a conversion factor that could be used to convert between moles of bromine monofluoride and moles of bromine pentafluoride.
f. How many moles of bromine monofluoride must react to yield 0.78 mole of bromine pentafluoride?

Lottie Adams
Lottie Adams
Numerade Educator
01:46

Problem 29

Potassium chlorate, $\mathrm{KClO}_3$, acts as an oxidizing agent in matches, explosives, flares, and fireworks. In the equation below, it is formed from the element chlorine and potassium hydroxide.

$$
3 \mathrm{Cl}_2+6 \mathrm{KOH} \rightarrow \mathrm{KClO}_3+5 \mathrm{KCl}+3 \mathrm{H}_2 \mathrm{O}
$$

a. Write a conversion factor that could be used to convert between moles of potassium hydroxide and moles of potassium chlorate.
b. How many moles of potassium chlorate form when 2 moles of potassium hydroxide react completely?
c. What is the maximum number of moles of $\mathrm{KClO}_3$ that could form in the combination of 6.0 moles of $\mathrm{Cl}_2$ with 9.0 moles of KOH ?
d. Write a conversion factor that could be used to convert between moles of chlorine and moles of potassium chloride.
e. How many moles of chlorine react when 2.006 moles of potassium chloride form?

Lottie Adams
Lottie Adams
Numerade Educator
04:56

Problem 30

Potassium perchlorate, $\mathrm{KClO}_4$, is a better oxidizing agent than the potassium chlorate, $\mathrm{KClO}_3$, described in the previous problem. Potassium perchlorate, which is used in explosives, fireworks, flares, and solid rocket propellants, is made by carefully heating potassium chlorate to between $400^{\circ} \mathrm{C}$ and $500^{\circ} \mathrm{C}$. The unbalanced equation for this reaction is

$$
\mathrm{KClO}_3 \rightarrow \mathrm{KClO}_4+\mathrm{KCl}
$$

a. Balance this equation.
b. Write a conversion factor that could be used to convert between moles of potassium chlorate and moles of potassium perchlorate.
c. How many moles of potassium perchlorate form from the complete reaction of 12 moles of potassium chlorate?
d. Write a conversion factor that could be used to convert between moles of potassium perchlorate and moles of potassium chloride.
e. How many moles of potassium chloride form along with 11.875 moles of potassium perchlorate?

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
11:27

Problem 31

Aniline, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_2$, is used to make many different chemicals, including dyes, photographic chemicals, antioxidants, explosives, and herbicides. It can be formed from nitrobenzene, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NO}_2$, in the following reaction with iron(II) chloride as a catalyst.

$$
4 \mathrm{C}_6 \mathrm{H}_5 \mathrm{NO}_2+9 \mathrm{Fe}+4 \mathrm{H}_2 \mathrm{O} \xrightarrow{\mathrm{FeCl}_2} 4 \mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_2+3 \mathrm{Fe}_3 \mathrm{O}_4
$$

a. Write a conversion factor that could be used to convert between moles of iron and moles of nitrobenzene.
b. What is the minimum mass of iron that would be necessary to react completely with 810.5 g of nitrobenzene, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NO}_2$ ?
c. Write a conversion factor that could be used to convert between moles of aniline and moles of nitrobenzene.
d. What is the maximum mass of aniline, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_2$, that can be formed from 810.5 g of nitrobenzene, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NO}_2$, with excess iron and water?
e. Write a conversion factor that could be used to convert between moles of $\mathrm{Fe}_3 \mathrm{O}_4$ and moles of aniline.
f. What is the mass of $\mathrm{Fe}_3 \mathrm{O}_4$ formed with the amount of aniline, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_2$, calculated in part (d)?
g. If 478.2 g of aniline, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_2$, are formed from the reaction of 810.5 g of nitrobenzene, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NO}_2$, with excess iron and water, what is the percent yield?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:05

Problem 32

Tetraboron carbide, $\mathrm{B}_4 \mathrm{C}$, is a very hard substance used for grinding purposes, ceramics, and armor plating. Because boron is an efficient absorber of neutrons, $\mathrm{B}_4 \mathrm{C}$ is also used as a protective material in nuclear reactors. The reaction that forms $\mathrm{B}_4 \mathrm{C}$ from boron(III) oxide, $\mathrm{B}_2 \mathrm{O}_3$, is

$$
2 \mathrm{~B}_2 \mathrm{O}_3+7 \mathrm{C} \xrightarrow{2400^{\circ} \mathrm{C}} \mathrm{~B}_4 \mathrm{C}+6 \mathrm{CO}
$$

a. Write a conversion factor that could be used to convert between moles of carbon and moles of boron(III) oxide.
b. What is the minimum mass of carbon, in grams, necessary to react completely with 24.675 g of boron(III) oxide, $\mathrm{B}_2 \mathrm{O}_3$ ?
c. Write a conversion factor that could be used to convert between moles of $\mathrm{B}_4 \mathrm{C}$ and moles of boron(III) oxide.
d. What is the maximum mass, in grams, of $\mathrm{B}_4 \mathrm{C}$ that can be formed from the reaction of 24.675 g of boron(III) oxide, $\mathrm{B}_2 \mathrm{O}_3$ with an excess of carbon?
e. If 9.210 g of $\mathrm{B}_4 \mathrm{C}$ is isolated in the reaction of 24.675 g of boron(III) oxide, $\mathrm{B}_2 \mathrm{O}_3$, with an excess of carbon, what is the percent yield?

Lottie Adams
Lottie Adams
Numerade Educator
05:27

Problem 33

Because of its red-orange color, sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, has been used in the manufacture of pigments. It can be made by reacting sodium chromate, $\mathrm{Na}_2 \mathrm{CrO}_4$, with sulfuric acid. The products other than sodium dichromate are sodium sulfate and water.
a. Write a balanced equation for this reaction. (You do not need to write the states.)
b. How many kilograms of sodium chromate, $\mathrm{Na}_2 \mathrm{CrO}_4$, are necessary to produce 84.72 kg of sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$ ?
c. How many kilograms of sodium sulfate are formed with 84.72 kg of $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$ ?

Niamat Khuda
Niamat Khuda
Numerade Educator
04:20

Problem 34

Chromium(III) oxide, often called chromic oxide, has been used as a green paint pigment, as a catalyst in organic synthesis, as a polishing powder, and to make metallic chromium. One way to make chromium(III) oxide is by reacting sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, with ammonium chloride at 800 to $1000{ }^{\circ} \mathrm{C}$ to form chromium(III) oxide, sodium chloride, nitrogen, and water.
a. Write a balanced equation for this reaction. (You do not need to write the states.)
b. What is the minimum mass, in megagrams, of ammonium chloride necessary to react completely with 275 Mg of sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$ ?
c. What is the maximum mass, in megagrams, of chromium(III) oxide that can be made from 275 Mg of sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, and excess ammonium chloride?
d. If 147 Mg of chromium(III) oxide is formed in the reaction of 275 Mg of sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, with excess ammonium chloride, what is the percent yield?

William Mills
William Mills
Numerade Educator
02:32

Problem 35

The tanning agent, $\mathrm{Cr}(\mathrm{OH}) \mathrm{SO}_4$, is formed in the reaction of sodium dichromate $\left(\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7\right)$, sulfur dioxide, and water. Tanning protects animal hides from bacterial attack, reduces swelling, and prevents the fibers from sticking together when the hides dry. This leads to a softer, more flexible leather.

$$
\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7+3 \mathrm{SO}_2+\mathrm{H}_2 \mathrm{O} \rightarrow 2 \mathrm{Cr}(\mathrm{OH}) \mathrm{SO}_4+\mathrm{Na}_2 \mathrm{SO}_4
$$

a. How many kilograms of sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, are necessary to produce 2.50 kg of $\mathrm{Cr}(\mathrm{OH}) \mathrm{SO}_4$ ?
b. How many megagrams of sodium sulfate are formed with 2.50 Mg of $\mathrm{Cr}(\mathrm{OH}) \mathrm{SO}_4$ ?

Angelina Chavez
Angelina Chavez
Numerade Educator
05:15

Problem 36

The mineral hausmannite, $\mathrm{Mn}_3 \mathrm{O}_4$, which contains both manganese(II) and manganese(III) ions, is formed from heating manganese(IV) oxide to $890^{\circ} \mathrm{C}$.

$$
3 \mathrm{MnO}_2(l) \xrightarrow{800^{\circ} \mathrm{C}} \mathrm{Mn}_3 \mathrm{O}_4(\mathrm{~s})+\mathrm{O}_2(\mathrm{~g})
$$

a. What is the maximum mass, in megagrams, of $\mathrm{Mn}_3 \mathrm{O}_4$ that can be formed from the decomposition of 31.85 Mg of manganese(IV) oxide, $\mathrm{MnO}_2$ ?
b. If 24.28 Mg of $\mathrm{Mn}_3 \mathrm{O}_4$ is isolated in the decomposition reaction of 31.85 Mg of manganese(IV) oxide, $\mathrm{MnO}_2$, what is the percent yield?

Katherine Mccandless
Katherine Mccandless
Numerade Educator
04:26

Problem 37

Describe four reasons for adding an excess of one or more of the reactants in a chemical reaction.

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
04:39

Problem 38

Chromium(III) oxide can be made from the reaction of sodium dichromate and ammonium chloride. What is the maximum mass, in grams, of chromium(III) oxide that can be produced from the complete reaction of 123.5 g of sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, with 59.5 g of ammonium chloride? The other products are sodium chloride, nitrogen gas, and water.

Marietjie Lutz
Marietjie Lutz
Numerade Educator
02:53

Problem 39

The equation for one process for making aluminum fluoride follows. What is the maximum mass, in grams, of aluminum fluoride, $\mathrm{AlF}_3$, that can be produced from the complete reaction of $1.4 \times 10^3 \mathrm{~g}$ of aluminum hydroxide, $\mathrm{Al}(\mathrm{OH})_3$, with $1.0 \times 10^3 \mathrm{~g}$ of $\mathrm{H}_2 \mathrm{SiF}_6$ ?

$$
2 \mathrm{Al}(\mathrm{OH})_3+\mathrm{H}_2 \mathrm{SiF}_6 \xrightarrow{100^{\circ} \mathrm{C}} 2 \mathrm{AlF}_3+\mathrm{SiO}_2+4 \mathrm{H}_2 \mathrm{O}
$$

Crystal Wang
Crystal Wang
Numerade Educator
10:02

Problem 40

Tetraboron carbide, $\mathrm{B}_4 \mathrm{C}$, which is used as a protective material in nuclear reactors, can be made from boric acid, $\mathrm{H}_3 \mathrm{BO}_3$.

$$
4 \mathrm{H}_3 \mathrm{BO}_3+7 \mathrm{C} \xrightarrow{2400^{\circ} \mathrm{C}} \mathrm{~B}_4 \mathrm{C}+6 \mathrm{CO}+6 \mathrm{H}_2 \mathrm{O}
$$

a. What is the maximum mass, in kilograms, of $\mathrm{B}_4 \mathrm{C}$ formed in the reaction of 30.0 kg of carbon with 54.785 kg of $\mathrm{H}_3 \mathrm{BO}_3$ ?
b. Explain why one of the substances in part (a) is in excess and one is limiting.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
05:18

Problem 41

Potassium permanganate, $\mathrm{KMnO}_4$, a common oxidizing agent, is made from various ores that contain manganese(IV) oxide, $\mathrm{MnO}_2$. The following equation shows the net reaction for one process that forms potassium permanganate.

$$
2 \mathrm{MnO}_2+2 \mathrm{KOH}+\mathrm{O}_2 \rightarrow 2 \mathrm{KMnO}_4+\mathrm{H}_2
$$

a. What is the maximum mass, in kilograms, of $\mathrm{KMnO}_4$ that can be made from the reaction of 835.6 g of $\mathrm{MnO}_2$ with 585 g of KOH and excess oxygen gas?
b. Explain why the oxygen gas is in excess.
c. If 1.18 kg of $\mathrm{KMnO}_4$ are isolated from the product mixture of the reaction of 835.6 g of $\mathrm{MnO}_2$ with 585 g of KOH and excess oxygen gas, what is the percent yield?

Ronald Prasad
Ronald Prasad
Numerade Educator
05:42

Problem 42

Aniline, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_2$, which is used to make antioxidants, can be formed from nitrobenzene, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NO}_2$, in the following reaction.

$$
4 \mathrm{C}_6 \mathrm{H}_5 \mathrm{NO}_2+9 \mathrm{Fe}+4 \mathrm{H}_2 \mathrm{O} \xrightarrow{\mathrm{FeCl}_2} 4 \mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_2+3 \mathrm{Fe}_3 \mathrm{O}_4
$$

a. What is the maximum mass of aniline, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_2$, formed in the reaction of 810.5 g of nitrobenzene, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{NO}_2$, with 985.0 g of Fe and 250 g of $\mathrm{H}_2 \mathrm{O}$ ?
b. Explain why two of these substances are in excess and one is limiting.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:08

Problem 43

Uranium is distributed in a form called yellow cake, which is made from uranium ore. In the second step of the reactions that form yellow cake from uranium ore, uranyl sulfate, $\mathrm{UO}_2 \mathrm{SO}_4$, is converted to $\left(\mathrm{NH}_4\right)_2 \mathrm{U}_2 \mathrm{O}_7$.

$$
2 \mathrm{UO}_2 \mathrm{SO}_4+6 \mathrm{NH}_3+3 \mathrm{H}_2 \mathrm{O} \rightarrow\left(\mathrm{NH}_4\right)_2 \mathrm{U}_2 \mathrm{O}_7+2\left(\mathrm{NH}_4\right)_2 \mathrm{SO}_4
$$

a. What is the maximum mass, in kilograms, of $\left(\mathrm{NH}_4\right)_2 \mathrm{U}_2 \mathrm{O}_7$ that can be formed from the reaction of 100 kg of water and 100 kg of ammonia with 481 kg of $\mathrm{UO}_2 \mathrm{SO}_4$ ?
b. Explain why two of these substances are in excess and one is limiting.

Reed Mckee
Reed Mckee
Numerade Educator
05:00

Problem 44

Calcium carbide, $\mathrm{CaC}_2$, is formed in the reaction between calcium oxide and carbon. The other product is carbon monoxide.
a. Write a balanced equation for this reaction. (You do not need to write the states.)
b. If you were designing the procedure for producing calcium carbide from calcium oxide and carbon, which of the reactants would you have as the limiting reactant? Why?
c. Assuming $100 \%$ yield from the limiting reactant, what are the approximate amounts of CaO and carbon that you would combine to form 860.5 g of $\mathrm{CaC}_2$ ?

DB
Dennis Burkett
Numerade Educator
06:58

Problem 45

Calcium carbide, $\mathrm{CaC}_2$, reacts with water to form acetylene, $\mathrm{C}_2 \mathrm{H}_2$, and calcium hydroxide.
a. Write a balanced equation for this reaction. (You do not need to write the states.)
b. If you were designing the procedure for producing acetylene from calcium carbide and water, which of the reactants would you have as the limiting reactant? Why?
c. Assuming $100 \%$ yield from the limiting reactant, what are the approximate amounts of $\mathrm{CaC}_2$ and water that you would combine to form 127 g of $\mathrm{C}_2 \mathrm{H}_2$ ?

Matthew Lueckheide
Matthew Lueckheide
Numerade Educator
02:59

Problem 46

Give four reasons why the actual yield in a chemical reaction is less than the theoretical yield.

David Alvarez-Carbonell
David Alvarez-Carbonell
Numerade Educator
03:54

Problem 47

When determining the theoretical yield for a reaction, why must we first determine which reactant is the limiting reactant?

Shazia Naz
Shazia Naz
Numerade Educator
06:31

Problem 48

Does the reactant in excess affect the actual yield for a reaction? If it does, explain how.

Kevin Chimex
Kevin Chimex
Numerade Educator
02:13

Problem 49

Can the calculated percent yield ever be above $100 \%$. If it can, explain how.

David Alvarez-Carbonell
David Alvarez-Carbonell
Numerade Educator
01:28

Problem 50

What is the molarity of a solution made by dissolving 37.452 g of aluminum sulfate, $\mathrm{Al}_2\left(\mathrm{SO}_4\right)_3$, in water and diluting with water to 250.0 mL total?

Eileen Sullivan
Eileen Sullivan
Numerade Educator
02:53

Problem 51

What is the molarity of a solution made by dissolving 18.476 g of potassium carbonate, $\mathrm{K}_2 \mathrm{CO}_3$, in water and diluting with water to 100.0 mL total?

Bhumika Jayee
Bhumika Jayee
Numerade Educator
10:29

Problem 52

The following equation represents the first step in the conversion of $\mathrm{UO}_3$, found in uranium ore, into the uranium compounds called "yellow cake."

$$
\mathrm{UO}_3+\mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{UO}_2 \mathrm{SO}_4+\mathrm{H}_2 \mathrm{O}
$$

a. How many milliliters of $18.0 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ are necessary to react completely with 249.6 g of $\mathrm{UO}_3$ ?
b. What is the maximum mass, in grams, of $\mathrm{UO}_2 \mathrm{SO}_4$ that forms from the complete reaction of 125 mL of $18.0 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ ?

Marissa Turner
Marissa Turner
Numerade Educator
02:40

Problem 53

Most of the sodium chlorate, $\mathrm{NaClO}_3$, produced in the United States is converted into chlorine dioxide, which is then used for bleaching wood pulp.

$$
\mathrm{NaClO}_3(a q)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{ClO}_2(g)+1 / 2 \mathrm{Cl}_2(g)+\mathrm{NaCl}(a q)+\mathrm{H}_2 \mathrm{O}(l)
$$

a. How many milliliters of 12.1 M HCl are necessary to react completely with 35.09 g of sodium chlorate, $\mathrm{NaClO}_3$ ?
b. What is the maximum mass, in grams, of $\mathrm{ClO}_2$ that can be formed from the complete reaction of 65 mL of 12.1 M HCl ?

Adriano Chikande
Adriano Chikande
Numerade Educator
06:20

Problem 54

When a water solution of sodium sulfite, $\mathrm{Na}_2 \mathrm{SO}_3$, is added to a water solution of iron(II) chloride, $\mathrm{FeCl}_2$, iron(II) sulfite, $\mathrm{FeSO}_3$, precipitates from the solution.
a. Write a balanced equation for this reaction.
b. What is the maximum mass of iron(II) sulfite that will precipitate from a solution prepared by adding an excess of a $\mathrm{Na}_2 \mathrm{SO}_3$ solution to 25.00 mL of $1.009 \mathrm{M} \mathrm{FeCl}_2$ ?

Ronald Prasad
Ronald Prasad
Numerade Educator
View

Problem 55

Consider the precipitation reaction that takes place when a water solution of aluminum nitrate, $\mathrm{Al}\left(\mathrm{NO}_3\right)_3$, is added to a water solution of potassium phosphate, $\mathrm{K}_3 \mathrm{PO}_4$.
a. Write a balanced equation for this reaction.
b. What is the maximum mass of aluminum phosphate that will precipitate from a solution prepared by adding an excess of an $\mathrm{Al}\left(\mathrm{NO}_3\right)_3$ solution to 50.00 mL of $1.525 \mathrm{M} \mathrm{K}_3 \mathrm{PO}_4$ ?

Tanvi Garg
Tanvi Garg
Numerade Educator
02:10

Problem 56

Consider the neutralization reaction that takes place when nitric acid reacts with aqueous potassium hydroxide.
a. Write a conversion factor that relates moles of $\mathrm{HNO}_3$ to moles of KOH for this reaction.
b. What is the minimum volume of $1.50 \mathrm{M} \mathrm{HNO}_3$ necessary to neutralize completely the hydroxide in 125.0 mL of 0.501 M KOH ?

Christopher Nilsen
Christopher Nilsen
Numerade Educator
05:13

Problem 57

Consider the neutralization reaction that takes place when hydrochloric acid reacts with aqueous sodium hydroxide.
a. Write a conversion factor that relates moles of HCl to moles of NaOH for this reaction.
b. What is the minimum volume of 6.00 M HCl necessary to neutralize completely the hydroxide in 750.0 mL of 0.107 M NaOH ?

David Collins
David Collins
Numerade Educator
03:36

Problem 58

Consider the neutralization reaction that takes place when sulfuric acid reacts with aqueous sodium hydroxide.
a. Write a conversion factor that relates moles of $\mathrm{H}_2 \mathrm{SO}_4$ to moles of NaOH for this reaction.
b. What is the minimum volume of $6.02 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ necessary to neutralize completely the hydroxide in 47.5 mL of 2.5 M NaOH ?

Freddie Montague
Freddie Montague
Numerade Educator
03:44

Problem 59

Consider the neutralization reaction that takes place when phosphoric acid reacts with aqueous potassium hydroxide.
a. Write a conversion factor that relates moles of $\mathrm{H}_3 \mathrm{PO}_4$ to moles of KOH for this reaction.
b. What is the minimum volume of $2.02 \mathrm{M} \mathrm{H}_3 \mathrm{PO}_4$ necessary to neutralize completely the hydroxide in 183 mL of 0.550 M KOH ?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:34

Problem 60

Consider the neutralization reaction that takes place when hydrochloric acid reacts with solid cobalt(II) hydroxide.
a. Write a conversion factor that relates moles of HCl to moles of $\mathrm{Co}(\mathrm{OH})_2$ for this reaction.
b. What is the minimum volume of 6.14 M HCl necessary to react completely with 2.53 kg of solid cobalt(II) hydroxide, $\mathrm{Co}(\mathrm{OH})_2$ ?

Heather Gamble
Heather Gamble
Numerade Educator
View

Problem 61

Consider the neutralization reaction that takes place when hydrochloric acid reacts with solid nickel(II) carbonate.
a. Write a conversion factor that relates moles of HCl to moles of $\mathrm{NiCO}_3$ for this reaction.
b. What is the minimum volume of 6.0 M HCl necessary to react completely with 14.266 g of solid nickel(II) carbonate, $\mathrm{NiCO}_3$ ?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:21

Problem 62

Consider the neutralization reaction that takes place when nitric acid reacts with solid chromium(III) hydroxide.
a. Write a conversion factor that relates moles of $\mathrm{HNO}_3$ to moles of $\mathrm{Cr}(\mathrm{OH})_3$ for this reaction.
b. What is the minimum volume of $2.005 \mathrm{M} \mathrm{HNO}_3$ necessary to react completely with 0.5187 kg of solid chromium(III) hydroxide, $\mathrm{Cr}(\mathrm{OH})_3$ ?

Sima Sarker
Sima Sarker
Numerade Educator
01:13

Problem 63

Consider the neutralization reaction that takes place when nitric acid reacts with solid iron(II) carbonate.
a. Write a conversion factor that relates moles of $\mathrm{HNO}_3$ to moles of $\mathrm{FeCO}_3$ for this reaction.
b. What is the minimum volume of $2.00 \mathrm{M} \mathrm{HNO}_3$ necessary to react completely with 1.06 kg of solid iron(II) carbonate, $\mathrm{FeCO}_3$ ?

David Collins
David Collins
Numerade Educator
View

Problem 64

Because nitrogen and phosphorus are both nonmetallic elements in group 15 on the periodic table, we expect them to react with other elements in similar ways. To some extent, they do, but there are also distinct differences in their chemical behavior. For example, nitrogen atoms form stable triple bonds to carbon atoms in substances such as hydrogen cyanide (often called hydrocyanic acid), HCN . Phosphorus atoms also form triple bonds to carbon atoms, in substances such as HCP, but those substances are much less stable. The compound HCP can be formed in the following reaction.

$$
\mathrm{CH}_4+\mathrm{PH}_3 \xrightarrow{\text { electric arc }} \mathrm{HCP}+3 \mathrm{H}_2
$$

a. Write a conversion factor that could be used to convert between moles of HCP and moles of $\mathrm{H}_2$.
b. How many moles of HCP form along with 9 moles of $\mathrm{H}_2$ ?
c. Write a conversion factor that could be used to convert between moles of methane, $\mathrm{CH}_4$, and moles of hydrogen, $\mathrm{H}_2$.
d. How many moles of hydrogen gas form when 1.8834 moles of $\mathrm{CH}_4$ react with an excess of $\mathrm{PH}_3$ ?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
05:09

Problem 65

Because carbon and silicon are both elements in group 14 on the periodic table, we expect them to react with other elements in similar ways. To some extent, they do, but in some cases, carbon and silicon compounds that seem to have analogous structures have very different chemical characteristics. For example, carbon tetrachloride, $\mathrm{CCl}_4$, is very stable in the presence of water, but silicon tetrachloride, $\mathrm{SiCl}_4$, reacts quickly with water. The unbalanced equation for this reaction is

$$
\mathrm{SiCl}_4+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{Si}(\mathrm{OH})_4+\mathrm{HCl}
$$

a. Balance this equation.
b. Write a conversion factor that could be used to convert between moles of $\mathrm{SiCl}_4$ and moles of $\mathrm{H}_2 \mathrm{O}$.
c. How many moles of $\mathrm{SiCl}_4$ react with 24 moles of water?
d. Write a conversion factor that could be used to convert between moles of $\mathrm{Si}(\mathrm{OH})_4$ and moles of water.
e. How many moles of $\mathrm{Si}(\mathrm{OH})_4$ form when 4.01 moles of $\mathrm{H}_2 \mathrm{O}$ react with an excess of $\mathrm{SiCl}_4$ ?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
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Problem 66

Iodine pentafluoride is an incendiary agent, a substance that ignites combustible materials. This compound is usually made by passing fluorine gas over solid iodine, but it also forms when iodine monofluoride changes into the element iodine and iodine pentafluoride.
a. Write a balanced equation, without including states, for the conversion of iodine monofluoride into iodine and iodine pentafluoride.
b. How many moles of the element iodine form when 15 moles of iodine monofluoride react completely?
c. How many moles of iodine pentafluoride form when 7.939 moles of iodine monofluoride react completely?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
09:52

Problem 67

The first laboratory experiments to produce compounds containing noble gas atoms aroused great excitement, not because the compounds might be useful but because they demonstrated that the noble gases were not completely inert. Since that time, however, important uses have been found for a number of noble gas compounds. For example, xenon difluoride, $\mathrm{XeF}_2$, is an excellent fluorinating agent (a substance that adds fluorine atoms to other substances). One reason it is preferred over certain other fluorinating agents is that the products of its fluorinating reactions are easily separated from the gaseous xenon. The following unbalanced equation represents one such reaction:

$$
\mathrm{S}_3 \mathrm{O}_9+\mathrm{XeF}_2 \rightarrow \mathrm{~S}_2 \mathrm{O}_6 \mathrm{~F}_2+\mathrm{Xe}
$$

a. Balance this equation.
b. What is the minimum number of moles of $\mathrm{XeF}_2$ necessary to react with 4 moles of $\mathrm{S}_3 \mathrm{O}_9$ ?
c. What is the maximum number of moles of $\mathrm{S}_2 \mathrm{O}_6 \mathrm{~F}_2$ that can form from the complete reaction of 4 moles of $\mathrm{S}_3 \mathrm{O}_9$ and 7 moles of $\mathrm{XeF}_2$ ?
d. How many moles of xenon gas form from the complete reaction of 0.6765 mole of $\mathrm{S}_3 \mathrm{O}_9$ ?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:32

Problem 68

Xenon hexafluoride is a better fluorinating agent than the xenon difluoride described in the previous problem, but it must be carefully isolated from any moisture. This is because xenon hexafluoride reacts with water to form hydrogen fluoride (hydrogen monofluoride) and the dangerously explosive xenon trioxide.
a. Write a balanced equation, without including states, for the reaction of xenon hexafluoride and water to form xenon trioxide and hydrogen fluoride.
b. How many moles of hydrogen fluoride form when 0.50 mole of xenon hexafluoride reacts completely?
c. What is the maximum number of moles of xenon trioxide that can form in the combination of 7 moles of xenon hexafluoride and 18 moles of water?

Narayan Hari
Narayan Hari
Numerade Educator
04:55

Problem 69

It is fairly easy to make the fluorides of xenon by combining xenon gas with fluorine gas. Unfortunately, the products of the reaction- $\mathrm{XeF}_2, \mathrm{XeF}_4$, and $\mathrm{XeF}_6$-are difficult to separate. The percentage of $\mathrm{XeF}_2$ can be raised by adding a large excess of xenon and removing the product mixture soon after the reaction has begun. The percentage of $\mathrm{XeF}_6$ can be raised by running the reaction at 700 to $800^{\circ} \mathrm{C}$ in the presence of a nickel catalyst with a large excess of fluorine. If $\mathrm{XeF}_4$ is desired, a different reaction can be used. For example, $\mathrm{XeF}_4$ can be made from the reaction of xenon gas with dioxygen difluoride. The reaction also produces oxygen gas.
a. Write a balanced equation, including states, for the reaction of xenon gas and dioxygen difluoride gas to form xenon tetrafluoride gas and oxygen gas.
b. How many moles of xenon tetrafluoride form from 7.50 moles of dioxygen difluoride?
c. What is the maximum number of moles of xenon tetrafluoride gas that can form in the combination of 4.75 moles of xenon and 9.00 moles of dioxygen difluoride?

Joanna Josey
Joanna Josey
Numerade Educator
02:13

Problem 70

Hydriodic acid is produced industrially by the reaction of hydrazine, $\mathrm{N}_2 \mathrm{H}_4$, with iodine, $\mathrm{I}_2 . \mathrm{HI}(\mathrm{aq})$ is used to make iodine salts such as AgI , which are used to seed clouds to promote rain. What is the minimum mass of iodine, $\mathrm{I}_2$, necessary to react completely with 87.0 g of hydrazine, $\mathrm{N}_2 \mathrm{H}_4$ ?

$$
\mathrm{N}_2 \mathrm{H}_4+2 \mathrm{I}_2 \rightarrow 4 \mathrm{HI}+\mathrm{N}_2
$$

Ronald Prasad
Ronald Prasad
Numerade Educator
05:36

Problem 71

Calcium dihydrogen phosphate, which is used in the production of triple superphosphate fertilizers, can be formed from the reaction of apatite, $\mathrm{Ca}_5\left(\mathrm{PO}_4\right)_3 \mathrm{~F}$, with phosphoric acid. How many grams of calcium dihydrogen phosphate can be formed from 6.78 g of $\mathrm{Ca}_5\left(\mathrm{PO}_4\right)_3 \mathrm{~F}$ ?

$$
2 \mathrm{Ca}_5\left(\mathrm{PO}_4\right)_3 \mathrm{~F}+14 \mathrm{H}_3 \mathrm{PO}_4 \rightarrow 10 \mathrm{Ca}\left(\mathrm{H}_2 \mathrm{PO}_4\right)_2+2 \mathrm{HF}
$$

Ivan Kochetkov
Ivan Kochetkov
Numerade Educator
08:27

Problem 72

Because plants need nitrogen compounds, potassium compounds, and phosphorus compounds to grow, these are often added to the soil as fertilizers. Potassium sulfate, which is used to make fertilizers, is made industrially by reacting potassium chloride with sulfur dioxide gas, oxygen gas, and water. Hydrochloric acid is formed with the potassium sulfate.
a. Write a balanced equation for this reaction. (You do not need to include states.)
b. What is the maximum mass, in kilograms, of potassium sulfate that can be formed from $2.76 \times 10^5 \mathrm{~kg}$ of potassium chloride with excess sulfur dioxide, oxygen, and water?
c. If $2.94 \times 10^5 \mathrm{~kg}$ of potassium sulfate is isolated from the reaction of $2.76 \times 10^5 \mathrm{~kg}$ of potassium chloride, what is the percent yield?

Carlene Jimenez
Carlene Jimenez
Numerade Educator
01:58

Problem 73

Sodium hydrogen sulfate is used as a cleaning agent and as a flux (a substance that promotes the fusing of metals and prevents the formation of oxides). One of the ways in which sodium hydrogen sulfate is manufactured is by reacting sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, with sulfuric acid. This process also forms water and chromium(VI) oxide, $\mathrm{CrO}_3$.
a. Write a balanced equation for this reaction. (You do not need to include states.)
b. How many kilograms of sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, are necessary to produce 130.4 kg of sodium hydrogen sulfate?
c. How many kilograms of chromium(VI) oxide are formed when 130.4 kg of sodium hydrogen sulfate is made?
d. What is the minimum volume of $18.0 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ solution necessary to react with 874.0 kg of sodium dichromate?
e. What is the maximum mass of sodium hydrogen sulfate, $\mathrm{NaHSO}_4$, that can be formed from the reaction of 874.0 kg of sodium dichromate with 400.0 L of $18.0 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ ?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:47

Problem 74

The element phosphorus can be made by reacting carbon in the form of coke with calcium phosphate, $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$, which is found in phosphate rock.

$$
\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2+5 \mathrm{C} \rightarrow 3 \mathrm{CaO}+5 \mathrm{CO}+2 \mathrm{P}
$$

a. What is the minimum mass of carbon, C , necessary to react completely with 67.45 Mg of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$ ?
b. What is the maximum mass of phosphorus produced from the reaction of 67.45 Mg of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$ with an excess of carbon?
c. What mass of calcium oxide, CaO , is formed with the mass of phosphorus calculated in part (b)?
d. If 11.13 Mg of phosphorus is formed in the reaction of 67.45 Mg of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$ with an excess of carbon, what is the percent yield?

Ronald Prasad
Ronald Prasad
Numerade Educator
02:53

Problem 75

When coal is burned, the sulfur it contains is converted into sulfur dioxide. This $\mathrm{SO}_2$ is a serious pollutant, so it needs to be removed before it escapes from the stack of a coal fired plant. One way to remove the $\mathrm{SO}_2$ is to add limestone, which contains calcium carbonate, $\mathrm{CaCO}_3$, to the coal before it is burned. The heat of the burning coal converts the $\mathrm{CaCO}_3$ to calcium oxide, CaO . The calcium oxide reacts with the sulfur dioxide in the following reaction:

$$
2 \mathrm{CaO}+2 \mathrm{SO}_2+\mathrm{O}_2 \rightarrow 2 \mathrm{CaSO}_4
$$

The solid calcium sulfate does not escape from the stack as the gaseous sulfur dioxide would. What mass of calcium sulfate forms for each 1.00 Mg of $\mathrm{SO}_2$ removed by this technique?

Reed Mckee
Reed Mckee
Numerade Educator
01:53

Problem 76

Thionyl chloride, $\mathrm{SOCl}_2$, is a widely used source of chlorine in the formation of pesticides, pharmaceuticals, dyes, and pigments. It can be formed from disulfur dichloride in the following reaction.

$$
2 \mathrm{SO}_2+\mathrm{S}_2 \mathrm{Cl}_2+3 \mathrm{Cl}_2 \rightarrow 4 \mathrm{SOCl}_2
$$

If 1.140 kg of thionyl chloride is isolated from the reaction of 457.6 grams of disulfur dichloride, $\mathrm{S}_2 \mathrm{Cl}_2$, with excess sulfur dioxide and chlorine gas, what is the percent yield?

Alice .
Alice .
Numerade Educator
01:48

Problem 77

Chromium(III) oxide, which can be converted into metallic chromium, is formed in the following reaction:

$$
\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7+\mathrm{S} \xrightarrow{800-1000^{\circ} \mathrm{C}} \mathrm{Cr}_2 \mathrm{O}_3+\mathrm{Na}_2 \mathrm{SO}_4
$$

a. How many grams of chromium(III) oxide, $\mathrm{Cr}_2 \mathrm{O}_3$, are formed in the reaction of 981 g of sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, with 330 g of sulfur, S?
b. Explain why one of these substances is in excess and one is limiting.

Stephen Ho
Stephen Ho
Numerade Educator
00:52

Problem 78

Sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, is converted to chromium(III) sulfate, which is used in the tanning of animal hides. Sodium dichromate can be made by reacting sodium chromate, $\mathrm{Na}_2 \mathrm{CrO}_4$, with water and carbon dioxide.

$$
2 \mathrm{Na}_2 \mathrm{CrO}_4+\mathrm{H}_2 \mathrm{O}+2 \mathrm{CO}_2 \rightleftharpoons \mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7+2 \mathrm{NaHCO}_3
$$

a. Show that the sodium chromate is the limiting reactant when 87.625 g of $\mathrm{Na}_2 \mathrm{CrO}_4$ reacts with 10.008 g of water and excess carbon dioxide.
b. Explain why the carbon dioxide and water are in excess and sodium chromate is limiting.

Jacquelin Ho
Jacquelin Ho
Numerade Educator
01:29

Problem 79

What is the molarity of a solution made by dissolving 37.895 g of $\mathrm{CoCl}_2$ in water and diluting with water to 250.0 mL total?

David Collins
David Collins
Numerade Educator
04:01

Problem 80

What is the molarity of a solution made by dissolving 100.065 g of $\mathrm{SnBr}_2$ in water and diluting with water to 1.00 L total?

Anna D.
Anna D.
Numerade Educator
03:30

Problem 81

Sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, can be made by reacting sodium chromate, $\mathrm{Na}_2 \mathrm{CrO}_4$, with sulfuric acid.

$$
2 \mathrm{Na}_2 \mathrm{CrO}_4+\mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7+\mathrm{Na}_2 \mathrm{SO}_4+\mathrm{H}_2 \mathrm{O}
$$

a. What is the minimum volume of $18.0 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ necessary to react completely with 15.345 kg of sodium chromate, $\mathrm{Na}_2 \mathrm{CrO}_4$ ?
b. What is the maximum mass, in kilograms, of sodium dichromate that can be formed from the reaction of 203 L of $18.0 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ ?

Mena Botros
Mena Botros
Numerade Educator
01:26

Problem 82

A precipitation reaction takes place when a water solution of sodium carbonate, $\mathrm{Na}_2 \mathrm{CO}_3$, is added to a water solution of chromium(III) nitrate, $\mathrm{Cr}\left(\mathrm{NO}_3\right)_3$.
a. Write a balanced equation for this reaction.
b. What is the maximum mass of chromium(III) carbonate that will precipitate from a solution prepared by adding an excess of a $\mathrm{Na}_2 \mathrm{CO}_3$ solution to 10.00 mL of $0.100 \mathrm{M} \mathrm{Cr}\left(\mathrm{NO}_3\right)_3$ ?

Adriano Chikande
Adriano Chikande
Numerade Educator
01:36

Problem 83

A precipitation reaction takes place when a water solution of potassium phosphate, $\mathrm{K}_3 \mathrm{PO}_4$, is added to a water solution of cobalt(II) chloride, $\mathrm{CoCl}_2$.
a. Write a balanced equation for this reaction.
b. What is the maximum mass of cobalt(II) phosphate that will precipitate from a solution prepared by adding an excess of a $\mathrm{K}_3 \mathrm{PO}_4$ solution to 5.0 mL of $1.0 \mathrm{M} \mathrm{CoCl}_2$ ?

Dylan Gunawardene
Dylan Gunawardene
Numerade Educator
02:16

Problem 84

Consider the neutralization reaction between nitric acid and aqueous barium hydroxide.
a. Write a conversion factor that shows the ratio of moles of nitric acid to moles of barium hydroxide.
b. What volume of 1.09 M nitric acid would be necessary to neutralize the hydroxide in 25.00 mL of 0.159 M barium hydroxide?

Nicole Smina
Nicole Smina
Numerade Educator
02:14

Problem 85

Consider the neutralization reaction between sulfuric acid and aqueous lithium hydroxide.
a. Write a conversion factor that shows the ratio of moles of sulfuric acid to moles of lithium hydroxide.
b. What volume of 0.505 M sulfuric acid would be necessary to neutralize the hydroxide in 25.00 mL of 2.87 M lithium hydroxide?

Mehrnaz Siavoshi
Mehrnaz Siavoshi
Numerade Educator
01:44

Problem 86

Consider the neutralization reaction between hydrochloric acid and solid zine carbonate.
a. Write a conversion factor that shows the ratio of moles of hydrochloric acid to moles of zinc carbonate.
b. What volume of 0.500 M hydrochloric acid would be necessary to neutralize and dissolve 562 milligrams of solid zinc carbonate?

Ronald Prasad
Ronald Prasad
Numerade Educator
02:53

Problem 87

Consider the neutralization reaction between nitric acid and solid cadmium hydroxide.
a. Write a conversion factor that shows the ratio of moles of nitric acid to moles of cadmium hydroxide.
b. What volume of 3.00 M nitric acid would be necessary to neutralize and dissolve 2.56 kg of solid cadmium hydroxide?

Lottie Adams
Lottie Adams
Numerade Educator
08:34

Problem 88

A solution is made by adding 22.609 g of a solid that is $96.3 \% \mathrm{NaOH}$ to a beaker of water. What volume of $2.00 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ is necessary to neutralize the NaOH in this solution?

Zafar Haider
Zafar Haider
Numerade Educator
01:20

Problem 89

Potassium hydroxide can be purchased as a solid that is $88.0 \% \mathrm{KOH}$. What is the minimum mass of this solid necessary to neutralize all of the HCl in 25.00 mL of 3.50 M HCl ?

Crystal Wang
Crystal Wang
Numerade Educator
04:09

Problem 90

Aluminum sulfate, often called alum, is used in paper making to increase the paper's stiffness and smoothness and to help keep the ink from running. It is made from the reaction of sulfuric acid with the aluminum oxide found in bauxite ore. The products are aluminum sulfate and water. Bauxite ore is $30 \%$ to $75 \%$ aluminum oxide.
a. Write a balanced equation for this reaction. (You do not need to write the states.)
b. What is the maximum mass, in kilograms, of aluminum sulfate that could be formed from $2.3 \times 10^3$ kilograms of bauxite ore that is $62 \%$ aluminum oxide?

Catherine Lemar
Catherine Lemar
Numerade Educator
02:19

Problem 91

The element phosphorus can be made by reacting carbon in the form of coke with $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$ found in phosphate ore. When 8.0 Mg of ore that is $68 \%$ $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$ is combined with an excess of carbon in the form of coke, what is the maximum mass, in megagrams, of phosphorus that can be formed?

$$
\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2+5 \mathrm{C} \rightarrow 3 \mathrm{CaO}+5 \mathrm{CO}+2 \mathrm{P}
$$

Stephen Ho
Stephen Ho
Numerade Educator
04:27

Problem 92

Sodium tripolyphosphate (or STPP), $\mathrm{Na}_5 \mathrm{P}_3 \mathrm{O}_{10}$, is used in detergents. It is made by combining phosphoric acid with sodium carbonate at 300 to $500{ }^{\circ} \mathrm{C}$. What is the minimum mass, in kilograms, of sodium carbonate that would be necessary to react with excess phosphoric acid to make enough STPP to produce $1.025 \times 10^5 \mathrm{~kg}$ of a detergent that is $32 \% \mathrm{Na}_5 \mathrm{P}_3 \mathrm{O}_{10}$ ?

$$
6 \mathrm{H}_3 \mathrm{PO}_4+5 \mathrm{Na}_2 \mathrm{CO}_3 \rightarrow 2 \mathrm{Na}_5 \mathrm{P}_3 \mathrm{O}_{10}+9 \mathrm{H}_2 \mathrm{O}+5 \mathrm{CO}_2
$$

Aadit Sharma
Aadit Sharma
Numerade Educator
01:13

Problem 93

Hydrazine, $\mathrm{N}_2 \mathrm{H}_4$, is a liquid with many industrial purposes, including the synthesis of herbicides and pharmaceuticals. It is made from urea in the following reaction at $100^{\circ} \mathrm{C}$.

$$
\begin{aligned}
\mathrm{NH}_2 \mathrm{CONH}_2+\mathrm{NaOCl}+ & 2 \mathrm{NaOH} \\
& \rightarrow \mathrm{~N}_2 \mathrm{H}_4+\mathrm{NaCl}+\mathrm{Na}_2 \mathrm{CO}_3+\mathrm{H}_2 \mathrm{O}
\end{aligned}
$$

If the percent yield for the reaction is $90.6 \%$, how many kilograms of hydrazine, $\mathrm{N}_2 \mathrm{H}_4$, are formed from the reaction of 243.6 kg of urea, $\mathrm{NH}_2 \mathrm{CONH}_2$, with excess sodium hypochlorite and sodium hydroxide?

David Collins
David Collins
Numerade Educator
View

Problem 94

Urea, $\mathrm{NH}_2 \mathrm{CONH}_2$, is a common nitrogen source used in fertilizers. When urea is made industrially, its temperature must be carefully controlled because heat turns urea into biuret, $\mathrm{NH}_2 \mathrm{CONHCONH}_2$, a compound that is harmful to plants. Consider a pure sample of urea that has a mass of 92.6 kg . If $0.5 \%$ of the urea in this sample decomposes to form biuret, what mass, in grams, of $\mathrm{NH}_2 \mathrm{CONHCONH} \mathrm{H}_2$ will it contain?

$$
2 \mathrm{NH}_2 \mathrm{CONH}_2 \rightarrow \mathrm{NH}_2 \mathrm{CONHCONH}_2+\mathrm{NH}_3
$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
15:31

Problem 95

Chilean niter deposits are mostly sodium nitrate, but they also contain $0.3 \%$ iodine in the form of calcium iodate, $\mathrm{Ca}\left(\mathrm{IO}_3\right)_2$. After the sodium nitrate in the niter is dissolved and recrystallized, the remaining solution contains $9 \mathrm{~g} / \mathrm{L}$ sodium iodate, $\mathrm{NaIO}_3(\mathrm{aq})$. The $\mathrm{NaIO}_3$ is converted to iodine when it reacts with sulfur dioxide and water.

$$
2 \mathrm{NaIO}_3+5 \mathrm{SO}_2+4 \mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{Na}_2 \mathrm{SO}_4+4 \mathrm{H}_2 \mathrm{SO}_4+\mathrm{I}_2
$$

a. How many liters of sodium iodate solution that contains 9 g of $\mathrm{NaIO}_3$ per liter would be necessary to form 127.23 kg of iodine, $\mathrm{I}_2$ ?
b. What mass, in megagrams, of Chilean niter that is $0.3 \%$ I would be necessary to form the volume of sodium iodate solution you calculated in part (a)?

Carolina Acevedo
Carolina Acevedo
Numerade Educator
01:58

Problem 96

The white pigment titanium(IV) oxide (often called titanium dioxide), $\mathrm{TiO}_2$, is made from rutile ore that is about $95 \% \mathrm{TiO}_2$. Before the $\mathrm{TiO}_2$ can be used, it must be purified. The equation that follows represents the first step in this purification.

$$
3 \mathrm{TiO}_2(\mathrm{~s})+4 \mathrm{C}(\mathrm{~s})+6 \mathrm{Cl}_2(\mathrm{~g}) \xrightarrow{900^{\circ} \mathrm{C}} 3 \mathrm{TiCl}_4(l)+2 \mathrm{CO}(\mathrm{~g})+2 \mathrm{CO}_2(\mathrm{~g})
$$

a. How many pounds of $\mathrm{TiCl}_4$ can be made from the reaction of $1.250 \times 10^5$ pounds of rutile ore that is $95 \% \mathrm{TiO}_2$ with $5.0 \times 10^4$ pounds of carbon?
b. Explain why two of these substances are in excess and one is limiting.

Ronald Prasad
Ronald Prasad
Numerade Educator
12:07

Problem 97

The tanning agent $\mathrm{Cr}(\mathrm{OH}) \mathrm{SO}_4$ is formed in the reaction of sodium dichromate, $\mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7$, sulfuric acid, and the sucrose in molasses:

$$
\begin{aligned}
8 \mathrm{Na}_2 \mathrm{Cr}_2 \mathrm{O}_7+24 & \mathrm{H}_2 \mathrm{SO}_4+\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11} \\
& \rightarrow 16 \mathrm{Cr}(\mathrm{OH}) \mathrm{SO}_4+8 \mathrm{Na}_2 \mathrm{SO}_4+12 \mathrm{CO}_2+22 \mathrm{H}_2 \mathrm{O}
\end{aligned}
$$

What is the maximum mass of $\mathrm{Cr}(\mathrm{OH}) \mathrm{SO}_4$ formed from the reaction of 431.0 kg of sodium dichromate with 292 L of $18.0 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ and 90.0 kg of $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$ ?

Riley Mankin
Riley Mankin
Numerade Educator
03:54

Problem 98

What is the maximum mass of calcium hydrogen phosphate, $\mathrm{CaHPO}_4$, that can form from the mixture of 12.50 kg of a solution that contains $84.0 \% \mathrm{H}_3 \mathrm{PO}_4$, 25.00 kg of $\mathrm{Ca}\left(\mathrm{NO}_3\right)_2, 25.00 \mathrm{~L}$ of $14.8 \mathrm{M} \mathrm{NH}_3$, and an excess of $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$ ?

$$
\begin{aligned}
3 \mathrm{H}_3 \mathrm{PO}_4+5 \mathrm{Ca}\left(\mathrm{NO}_3\right)_2 & +10 \mathrm{NH}_3+2 \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O} \\
& \rightarrow \quad 10 \mathrm{NH}_4 \mathrm{NO}_3+2 \mathrm{CaCO}_3+3 \mathrm{CaHPO}_4
\end{aligned}
$$

Ivan Kochetkov
Ivan Kochetkov
Numerade Educator