• Home
  • Textbooks
  • Introductory Chemistry
  • Quantities in Chemical Reactions

Introductory Chemistry

Nivaldo J. Tro

Chapter 8

Quantities in Chemical Reactions - all with Video Answers

Educators

+ 3 more educators

Chapter Questions

00:36

Problem 1

Why is reaction stoichiometry important? Cite some examples in your answer.

Carlene Jimenez
Carlene Jimenez
Numerade Educator
02:27

Problem 2

Nitrogen and hydrogen can react to form ammonia: $$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$$
(a) Write ratios showing the relationships between moles of each of the reactants and products in the reaction.
(b) How many molecules of $\mathrm{H}_{2}$ are required to completely react with two molecules of $\mathrm{N}_{2} ?$
(c) How many moles of $\mathrm{H}_{2}$ are required to completely react with 2 mol of $\mathrm{N}_{2}$ ?

Carlene Jimenez
Carlene Jimenez
Numerade Educator
02:02

Problem 3

Write the conversion factor that you would use to convert from moles of $\mathrm{Cl}_{2}$ to moles of $\mathrm{NaCl}$ in the reaction:
$$2 \mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NaCl}(s)$$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:44

Problem 4

What is wrong with this statement in reference to the reaction in the previous problem? "2 g of Na react with 1 g of $\mathrm{Cl}_{2}$ to form $2 \mathrm{g}$ of $\mathrm{NaCl}$." Correct the statement to make it true.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:06

Problem 5

What is the general form of the solution map for problems in which you are given the mass of a reactant in a chemical reaction and asked to find the mass of the product that can be made from the given amount of reactant?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
06:12

Problem 6

Consider the recipe for making tomato and garlic pasta.
2 cups noodles +12 tomatoes +3 cloves garlic $\longrightarrow 4$ servings pasta
If you have 7 cups of noodles, 27 tomatoes, and 9 cloves of garlic, how many servings of pasta can you make? Which ingredient limits the amount of pasta that it is possible to make?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:20

Problem 7

In a chemical reaction, what is the limiting reactant?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:30

Problem 8

In a chemical reaction, what is the theoretical yield?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:36

Problem 9

In a chemical reaction, what are the actual yield and percent yield?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
08:07

Problem 10

If you are given a chemical equation and specific amounts for each reactant in grams, how do you determine the maximum amount of product that can be made?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:57

Problem 11

Consider the generic chemical reaction: $$A+2 B \longrightarrow C+D$$ Suppose you have $12 \mathrm{g}$ of $\mathrm{A}$ and $24 \mathrm{g}$ of $\mathrm{B} .$ Which statement is true?
(a) A will definitely be the limiting reactant.
(b) B will definitely be the limiting reactant.
(c) A will be the limiting reactant if its molar mass is less than B.
(d) A will be the limiting reactant if its molar mass is greater than B.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
01:36

Problem 12

Consider the generic chemical equation: $$A+B \longrightarrow C$$ Suppose $25 \mathrm{g}$ of $\mathrm{A}$ were allowed to react with $8 \mathrm{g}$ of $\mathrm{B}$. Analysis of the final mixture showed that A was completely used up and 4 g of B remained. What was the limiting reactant?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:46

Problem 13

What is the enthalpy of reaction $\left(\Delta H_{\mathrm{rxn}}\right) ?$ Why is this quantity important?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:51

Problem 14

Explain the relationship between the sign of $\Delta H_{\mathrm{rxn}}$ and whether a reaction is exothermic or endothermic.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:20

Problem 15

Consider the generic chemical reaction: $$A+2 B \longrightarrow C$$ How many moles of $\mathrm{C}$ are formed upon complete reaction of:
(a) $2 \mathrm{mol}$ of $A$
(b) $2 \mathrm{mol}$ of $\mathrm{B}$
(c) $3 \mathrm{mol}$ of $A$
(d) $3 \mathrm{mol}$ of $\mathrm{B}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:29

Problem 16

Consider the generic chemical reaction: $$2 \mathrm{A}+3 \mathrm{B} \longrightarrow 3 \mathrm{C}$$
How many moles of $\mathrm{B}$ are required to completely react with:
(a) 6 mol of $A$
(b) 2 mol of $A$
(c) 7 mol of $A$
(d) 11 mol of $A$

Sima Sarker
Sima Sarker
Numerade Educator
03:44

Problem 17

For the reaction shown, calculate how many moles of $\mathrm{NO}_{2}$ form when each amount of reactant completely reacts. $$2 \mathrm{N}_{2} \mathrm{O}_{5}(g) \longrightarrow 4 \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g)$$
(a) $1.3 \mathrm{mol} \mathrm{N}_{2} \mathrm{O}_{5}$
(b) $5.8 \mathrm{mol} \mathrm{N}_{2} \mathrm{O}_{5}$
(c) $4.45 \times 10^{3} \mathrm{mol} \mathrm{N}_{2} \mathrm{O}_{5}$
(d) $1.006 \times 10^{-3} \mathrm{mol} \mathrm{N}_{2} \mathrm{O}_{5}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:56

Problem 18

For the reaction shown, calculate how many moles of $\mathrm{NH}_{3}$ form when each amount of reactant completely reacts. $$3 \mathrm{N}_{2} \mathrm{H}_{4}(l) \longrightarrow 4 \mathrm{NH}_{3}(g)+\mathrm{N}_{2}(g)$$
(a) $5.3 \mathrm{mol} \mathrm{N}_{2} \mathrm{H}_{4}$
(b) $2.28 \mathrm{mol} \mathrm{N}_{2} \mathrm{H}_{4}$
(c) $5.8 \times 10^{-2} \mathrm{mol} \mathrm{N}_{2} \mathrm{H}_{4}$
(d) $9.76 \times 10^{7} \mathrm{mol} \mathrm{N}_{2} \mathrm{H}_{4}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:23

Problem 19

Dihydrogen monosulfide reacts with sulfur dioxide according to the balanced equation:
$$2 \mathrm{H}_{2} \mathrm{S}(g)+\mathrm{SO}_{2}(g) \longrightarrow 3 \mathrm{S}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)$$ If the first figure represents the amount of $\mathrm{SO}_{2}$ available to react, which figure best represents the amount of $\mathrm{H}_{2} \mathrm{S}$ required to completely react with all of the $\mathrm{SO}_{2} ?$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:30

Problem 20

Chlorine gas reacts with fluorine gas according to the balanced equation: $$\mathrm{Cl}_{2}(g)+3 \mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{ClF}_{3}(g)$$ If the first figure represents the amount of fluorine available to react, and assuming that there is more than enough chlorine, which figure best represents the amount of chlorine trifluoride that would form upon complete reaction of all of the fluorine?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:30

Problem 21

For each reaction, calculate how many moles of product form when 1.75 mol of the reactant in color completely reacts. Assume there is more than enough of the other reactant.
(a) $\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{HCl}(g)$
(b) $2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)$
(c) $2 \mathrm{Na}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Na}_{2} \mathrm{O}_{2}(s)$
(d) $2 \mathrm{S}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:30

Problem 22

For each reaction, calculate how many moles of the product form when 0.112 mol of the reactant in color completely reacts. Assume there is more than enough of the other reactant.
(a) $2 \mathrm{Ca}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CaO}(s)$
(b) $4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)$
(c) $4 \mathrm{K}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{K}_{2} \mathrm{O}(s)$
(d) $4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(s)$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:58

Problem 23

For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume there is more than enough of the other reactant.
$$2 \mathrm{PbS}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{PbO}(s)+2 \mathrm{SO}_{2}(g)$$
(a) $2.4 \mathrm{mol} \mathrm{PbS}$
(b) $2.4 \mathrm{mol} \mathrm{O}_{2}$
(c) $5.3 \mathrm{mol} \mathrm{PbS}$
(d) $5.3 \mathrm{mol} \mathrm{O}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:27

Problem 24

For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume there is more than enough of the other reactant.
$$\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$$
(a) $4.6 \mathrm{mol} \mathrm{C}_{3} \mathrm{H}_{8}$
(b) $4.6 \mathrm{mol} \mathrm{O}_{2}$
(c) $0.0558 \mathrm{mol} \mathrm{C}_{3} \mathrm{H}_{8}$
(d) $0.0558 \mathrm{mol} \mathrm{O}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
06:02

Problem 25

Consider the balanced equation:
$$2 \mathrm{N}_{2} \mathrm{H}_{4}(g)+\mathrm{N}_{2} \mathrm{O}_{4}(g) \longrightarrow 3 \mathrm{N}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$$
Complete the table with the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product formed. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:40

Problem 26

Consider the balanced equation:
$$\mathrm{SiO}_{2}(s)+3 \mathrm{C}(s) \longrightarrow \mathrm{SiC}(s)+2 \mathrm{CO}(g)$$
Complete the table with the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product formed. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:52

Problem 27

Consider the unbalanced equation for the combustion of butane:
$$\mathrm{C}_{4} \mathrm{H}_{10}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$$
Balance the equation and determine how many moles of $\mathrm{O}_{2}$ are required to react completely with $4.9 \mathrm{mol}$ of $\mathrm{C}_{4} \mathrm{H}_{10}$.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:40

Problem 28

Consider the unbalanced equation for the neutralization of acetic acid:
$$\begin{aligned}\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow & \\ &\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Ca}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q) &\end{aligned}$$
Balance the equation and determine how many moles of $\mathrm{Ca}(\mathrm{OH})_{2}$ are required to completely neutralize $1.07 \mathrm{mol}$ of $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:49

Problem 29

Consider the unbalanced equation for the reaction of solid lead with silver nitrate:
$$\mathrm{Pb}(s)+\mathrm{AgNO}_{3}(a q) \longrightarrow \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Ag}(s)$$
(a) Balance the equation.
(b) How many moles of silver nitrate are required to completely react with 9.3 mol of lead?
(c) How many moles of Ag are formed by the complete reaction of 28.4 mol of $\mathrm{Pb}$ ?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:35

Problem 30

Consider the unbalanced equation for the reaction of aluminum with sulfuric acid:
$$\mathrm{Al}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+\mathrm{H}_{2}(g)$$
(a) Balance the equation.
(b) How many moles of $\mathrm{H}_{2} \mathrm{SO}_{4}$ are required to completely react with 8.3 mol of $\mathrm{Al} ?$
(c) How many moles of $\mathrm{H}_{2}$ are formed by the complete reaction of 0.341 mol of $\mathrm{Al} ?$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:29

Problem 31

For the reaction shown, calculate how many grams of oxygen form when each quantity of reactant completely reacts. $$2 \mathrm{HgO}(s) \longrightarrow 2 \mathrm{Hg}(l)+\mathrm{O}_{2}(g)$$
(a) $2.13 \mathrm{g} \mathrm{HgO}$
(b) $6.77 \mathrm{g} \mathrm{HgO}$
(c) $1.55 \mathrm{kg} \mathrm{HgO}$
(d) $3.87 \mathrm{mg} \mathrm{HgO}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
View

Problem 32

For the reaction shown, calculate how many grams of oxygen form when each quantity of reactant completely reacts. $$2 \mathrm{KClO}_{3}(s) \longrightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)$$
(a) $2.72 \mathrm{g} \mathrm{KClO}_{3}$
(b) $0.361 \mathrm{g} \mathrm{KClO}_{3}$
(c) $83.6 \mathrm{kg} \mathrm{KClO}_{3}$
(d) $22.4 \mathrm{mg} \mathrm{KClO}_{3}$

Ronald Prasad
Ronald Prasad
Numerade Educator
05:44

Problem 33

For each of the reactions, calculate how many grams of the product form when $2.4 \mathrm{g}$ of the reactant in color completely reacts. Assume there is more than enough of the other reactant.
(a) $2 \mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NaCl}(s)$
(b) $\operatorname{CaO}(s)+\mathrm{CO}_{2}(g) \longrightarrow \mathrm{CaCO}_{3}(s)$
(c) $2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MgO}(s)$
(d) $\mathrm{Na}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{NaOH}(a q)$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:14

Problem 34

For each of the reactions, calculate how many grams of the product form when $17.8 \mathrm{g}$ of the reactant in color completely reacts. Assume there is more than enough of the other reactant.
(a) $\mathrm{Ca}(\mathrm{s})+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CaCl}_{2}(\mathrm{s})$
(b) $2 \mathrm{K}(s)+\mathrm{Br}_{2}(l) \longrightarrow 2 \mathrm{KBr}(s)$
(c) $4 \mathrm{Cr}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Cr}_{2} \mathrm{O}_{3}(s)$
(d) $2 \operatorname{Sr}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \operatorname{SrO}(s)$

Hailey Tomashek
Hailey Tomashek
Numerade Educator
View

Problem 35

For the reaction shown, calculate how many grams of each product form when the given amount of each reactant completely reacts to form products. Assume there is more than enough of the other reactant. $$2 \mathrm{Al}(s)+\mathrm{Fe}_{2} \mathrm{O}_{3}(s) \longrightarrow \mathrm{Al}_{2} \mathrm{O}_{3}(s)+2 \mathrm{Fe}(l)$$
(a) $4.7 \mathrm{g} \mathrm{Al}$
(b) $4.7 \mathrm{g} \mathrm{Fe}_{2} \mathrm{O}_{3}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:17

Problem 36

For the reaction shown, calculate how many grams of each product form when the given amount of each reactant completely reacts to form products. Assume there is more than enough of the other reactant. $$\begin{aligned}2 \mathrm{HCl}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \rightarrow & \\& 2 \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g)\end{aligned}$$
(a) $10.8 \mathrm{g} \mathrm{HCl}$
(b) $10.8 \mathrm{g} \mathrm{Na}_{2} \mathrm{CO}_{3}$

Nicholas Mogoi
Nicholas Mogoi
Numerade Educator
10:38

Problem 37

Consider the balanced equation for the combustion of methane, a component of natural gas:
$$\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$$ Complete the table with the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that forms.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
View

Problem 38

Consider the balanced equation for the combustion of butane, a fuel often used in lighters:
$$2 \mathrm{C}_{4} \mathrm{H}_{10}(g)+13 \mathrm{O}_{2}(g) \longrightarrow 8 \mathrm{CO}_{2}(g)+10 \mathrm{H}_{2} \mathrm{O}(g)$$ Complete the table showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that forms.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:46

Problem 39

For each acid-base reaction, calculate how many grams of acid are necessary to completely react with and neutralize $2.5 \mathrm{g}$ of the base.
(a) $\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaCl}(a q)$
(b) $2 \mathrm{HNO}_{3}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow$
$2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(a q)$
(c) $\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{KOH}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:01

Problem 40

For each precipitation reaction, calculate how many grams of the first reactant are necessary to completely react with 17.3 g of the second reactant.
(a) $2 \mathrm{KI}(a q)+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow \mathrm{PbI}_{2}(s)+2 \mathrm{KNO}_{3}(a q)$
(b) $\mathrm{Na}_{2} \mathrm{CO}_{3}(a q)+\mathrm{CuCl}_{2}(a q) \longrightarrow \mathrm{CuCO}_{3}(s)+2 \mathrm{NaCl}(a q)$
(c) $\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow$ $\mathrm{SrSO}_{4}(s)+2 \mathrm{KNO}_{3}(a q)$

Oluwapelumi Kolawole
Oluwapelumi Kolawole
Numerade Educator
03:14

Problem 41

Sulfuric acid can dissolve aluminum metal according to the reaction:
$$2 \mathrm{Al}(s)+3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+3 \mathrm{H}_{2}(g)$$
Suppose you wanted to dissolve an aluminum block with a mass of $22.5 \mathrm{g}$. What minimum amount of $\mathrm{H}_{2} \mathrm{SO}_{4}$ in grams do you need? How many grams of $\mathrm{H}_{2}$ gas will be produced by the complete reaction of the aluminum block?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:20

Problem 42

Hydrochloric acid can dissolve solid iron according to the reaction:
$$\mathrm{Fe}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{FeCl}_{2}(a q)+\mathrm{H}_{2}(g)$$
What minimum mass of HCl in grams dissolves a $2.8-\mathrm{g}$ iron bar on a padlock? How much $\mathrm{H}_{2}$ is produced by the complete reaction of the iron bar?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:26

Problem 43

Consider the generic chemical equation: $$2 \mathrm{A}+4 \mathrm{B} \longrightarrow 3 \mathrm{C}$$
What is the limiting reactant when each of the initial quantities of $\mathrm{A}$ and $\mathrm{B}$ is allowed to react?
(a) 2 mol $A ; 5$ mol $B$
(b) $1.8 \mathrm{mol} \mathrm{A} ; 4 \mathrm{mol} \mathrm{B}$
(c) 3 mol $A ; 4$ mol $B$
(d) 22 mol $A ; 40$ mol $B$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:14

Problem 44

Consider the generic chemical equation: $$A+3 B \longrightarrow C$$
What is the limiting reactant when each of the initial quantities of $A$ and $B$ is allowed to react?
(a) 1 mol $A ; 4$ mol $B$
(b) 2 mol $A ; 3$ mol $B$
(c) 0.5 mol $A ; 1.6$ mol $B$
(d) 24 mol $A ; 75$ mol $B$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:28

Problem 45

Determine the theoretical yield of $C$ when each of the initial quantities of $\mathrm{A}$ and $\mathrm{B}$ is allowed to react in the generic reaction: $$A+2 B \longrightarrow 3 C$$
(a) 1 mol $A ; 1$ mol $B$
(b) $2 \mathrm{mol} \mathrm{A} ; 2 \mathrm{mol} \mathrm{B}$
(c) 1 mol $A ; 3$ mol $B$
(d) $32 \mathrm{mol} \mathrm{A} ; 68 \mathrm{mol} \mathrm{B}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:04

Problem 46

Determine the theoretical yield of $C$ when each of the initial quantities of $\mathrm{A}$ and $\mathrm{B}$ is allowed to react in the generic reaction: $$2 \mathrm{A}+3 \mathrm{B} \longrightarrow 2 \mathrm{C}$$
(a) 2 mol $A ; 4$ mol $B$
(b) $3 \mathrm{mol} \mathrm{A} ; 3 \mathrm{mol} \mathrm{B}$
(c) 5 mol $A ; 6$ mol $B$
(d) $4 \mathrm{mol} \mathrm{A} ; 5 \mathrm{mol} \mathrm{B}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:34

Problem 47

For the reaction shown, find the limiting reactant for each of the initial quantities of reactants.
$$2 \mathrm{K}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{KCl}(s)$$
(a) $1 \mathrm{mol} \mathrm{K} ; 1 \mathrm{mol} \mathrm{Cl}_{2}$
(b) $1.8 \mathrm{mol} \mathrm{K} ; 1 \mathrm{mol} \mathrm{Cl}_{2}$
(c) $2.2 \mathrm{mol} \mathrm{K} ; 1 \mathrm{mol} \mathrm{Cl}_{2}$
(d) $14.6 \mathrm{mol} \mathrm{K} ; 7.8 \mathrm{mol} \mathrm{Cl}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:59

Problem 48

For the reaction shown, find the limiting reactant for each of the initial quantities of reactants.
$$4 \mathrm{Cr}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Cr}_{2} \mathrm{O}_{3}(s)$$
(a) $1 \mathrm{mol} \mathrm{Cr} ; 1 \mathrm{mol} \mathrm{O}_{2}$
(b) $4 \mathrm{mol} \mathrm{Cr} ; 2.5 \mathrm{mol} \mathrm{O}_{2}$
(c) $12 \mathrm{mol} \mathrm{Cr} ; 10 \mathrm{mol} \mathrm{O}_{2}$
(d) $14.8 \mathrm{mol} \mathrm{Cr} ; 10.3 \mathrm{mol} \mathrm{O}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
07:04

Problem 49

For the reaction shown, calculate the theoretical yield of product in moles for each of the initial quantities of reactants. $$2 \mathrm{Mn}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MnO}_{3}(s)$$
(a) $2 \mathrm{mol} \mathrm{Mn} ; 2 \mathrm{mol} \mathrm{O}_{2}$
(b) $4.8 \mathrm{mol} \mathrm{Mn} ; 8.5 \mathrm{mol} \mathrm{O}_{2}$
(c) $0.114 \mathrm{mol} \mathrm{Mn} ; 0.161 \mathrm{mol} \mathrm{O}_{2}$
(d) $27.5 \mathrm{mol} \mathrm{Mn} ; 43.8 \mathrm{mol} \mathrm{O}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:26

Problem 50

For the reaction shown, calculate the theoretical yield of the product in moles for each of the initial quantities of reactants. $$\mathrm{Ti}(s)+2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{TiCl}_{4}(s)$$
(a) $2 \mathrm{mol} \mathrm{Ti} ; 2 \mathrm{mol} \mathrm{Cl}_{2}$
(b) $5 \mathrm{mol} \mathrm{Ti} ; 9 \mathrm{mol} \mathrm{Cl}_{2}$
(c) $0.483 \mathrm{mol} \mathrm{Ti} ; 0.911 \mathrm{mol} \mathrm{Cl}_{2}$
(d) $12.4 \mathrm{mol} \mathrm{Ti} ; 15.8 \mathrm{mol} \mathrm{Cl}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:36

Problem 51

Consider the generic reaction between reactants $A$ and $B$ :
$$3 \mathrm{A}+4 \mathrm{B} \longrightarrow 2 \mathrm{C}$$
If a reaction vessel initially contains 9 mol $A$ and 8 mol $B$, how many moles of $\mathrm{A}, \mathrm{B},$ and $\mathrm{C}$ will be in the reaction vessel after the reactants have reacted as much as possible? (Assume $100 \%$ actual yield.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:05

Problem 52

Consider the reaction between reactants $S$ and $O_{2}$ :
$$2 \mathrm{S}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)$$
If a reaction vessel initially contains 5 mol $S$ and 9 mol $\mathrm{O}_{2}$ how many moles of $S, O_{2},$ and $S O_{3}$ will be in the reaction vessel after the reactants have reacted as much as possible? (Assume $100 \%$ actual yield.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:15

Problem 53

Consider the reaction:
$$4 \mathrm{HCl}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)+2 \mathrm{Cl}_{2}(g)$$
Each molecular diagram represents an initial mixture of the reactants. How many molecules of $\mathrm{Cl}_{2}$ are formed by complete reaction in each case? (Assume $100 \%$ actual yield.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:08

Problem 54

Consider the reaction:
$$2 \mathrm{CH}_{3} \mathrm{OH}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$$
Each molecular diagram represents an initial mixture of the reactants. How many $\mathrm{CO}_{2}$ molecules are formed by complete reaction in each case? (Assume $100 \%$ actual yield.)

David Collins
David Collins
Numerade Educator
06:14

Problem 55

For the reaction shown, find the limiting reactant for each of the initial quantities of reactants.
$$2 \mathrm{Li}(s)+\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{LiF}(s)$$
(a) $1.0 \mathrm{g} \mathrm{Li} ; 1.0 \mathrm{g} \mathrm{F}_{2}$
(b) $10.5 \mathrm{g} \mathrm{Li} ; 37.2 \mathrm{g} \mathrm{F}_{2}$
(c) $2.85 \times 10^{3} \mathrm{g} \mathrm{Li} ; 6.79 \times 10^{3} \mathrm{g} \mathrm{F}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:07

Problem 56

For the reaction shown, find the limiting reactant for each of the initial quantities of reactants.
$$4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(s)$$
(a) $1.0 \mathrm{g} \mathrm{Al} ; 1.0 \mathrm{g} \mathrm{O}_{2}$
(b) $2.2 \mathrm{g} \mathrm{Al} ; 1.8 \mathrm{g} \mathrm{O}_{2}$
(c) $0.353 \mathrm{g} \mathrm{Al} ; 0.482 \mathrm{g} \mathrm{O}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
08:18

Problem 57

For the reaction shown, calculate the theoretical yield of the product in grams for each of the initial quantities of reactants. $$2 \mathrm{Al}(s)+3 \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{AlCl}_{3}(s)$$
(a) $1.0 \mathrm{g} \mathrm{Al} ; 1.0 \mathrm{g} \mathrm{Cl}_{2}$
(b) $5.5 \mathrm{g} \mathrm{Al} ; 19.8 \mathrm{g} \mathrm{Cl}_{2}$
(c) $0.439 \mathrm{g} \mathrm{Al} ; 2.29 \mathrm{g} \mathrm{Cl}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
07:21

Problem 58

For the reaction shown, calculate the theoretical yield of the product in grams for each of the initial quantities of reactants. $$\mathrm{Ti}(s)+2 \mathrm{F}_{2}(g) \longrightarrow \mathrm{TiF}_{4}(s)$$
(a) $1.0 \mathrm{g} \mathrm{Ti} ; 1.0 \mathrm{g} \mathrm{F}_{2}$
(b) $4.8 \mathrm{g} \mathrm{Ti} ; 3.2 \mathrm{g} \mathrm{F}_{2}$
(c) $0.388 \mathrm{g} \mathrm{Ti} ; 0.341 \mathrm{g} \mathrm{F}_{2}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:16

Problem 59

If the theoretical yield of a reaction is $24.8 \mathrm{g}$ and the actual yield is $18.5 \mathrm{g},$ what is the percent yield?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:26

Problem 60

If the theoretical yield of a reaction is 0.118 g and the actual yield is $0.104 \mathrm{g},$ what is the percent yield?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:27

Problem 61

Consider the reaction between calcium oxide and carbon dioxide:
$$\mathrm{CaO}(s)+\mathrm{CO}_{2}(g) \longrightarrow \mathrm{CaCO}_{3}(s)$$
A chemist allows $14.4 \mathrm{g}$ of $\mathrm{CaO}$ and $13.8 \mathrm{g}$ of $\mathrm{CO}_{2}$ to react. When the reaction is finished, the chemist collects $19.4 \mathrm{g}$ of $\mathrm{CaCO}_{3} .$ Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:02

Problem 62

Consider the reaction between sulfur trioxide and water:
$$\mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q)$$
A chemist allows $61.5 \mathrm{g}$ of $\mathrm{SO}_{3}$ and $11.2 \mathrm{g}$ of $\mathrm{H}_{2} \mathrm{O}$ to react. When the reaction is finished, the chemist collects $54.9 \mathrm{g}$ of $\mathrm{H}_{2} \mathrm{SO}_{4}$. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
07:12

Problem 63

Consider the reaction between $\mathrm{NiS}_{2}$ and $\mathrm{O}_{2}$ :
$$2 \mathrm{NiS}_{2}(s)+5 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NiO}(s)+4 \mathrm{SO}_{2}(g)$$
When $11.2 \mathrm{g}$ of $\mathrm{NiS}_{2}$ react with $5.43 \mathrm{g}$ of $\mathrm{O}_{2}, 4.86 \mathrm{g}$ of $\mathrm{NiO}$ are obtained. Determine the limiting reactant, theoretical yield of $\mathrm{NiO},$ and percent yield for the reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:40

Problem 64

Consider the reaction between $\mathrm{HCl}$ and $\mathrm{O}_{2}$ :
$$4 \mathrm{HCl}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{Cl}_{2}(g)$$
When $63.1 \mathrm{g}$ of $\mathrm{HCl}$ react with $17.2 \mathrm{g}$ of $\mathrm{O}_{2}, 49.3 \mathrm{g}$ of $\mathrm{Cl}_{2}$ are collected. Determine the limiting reactant, theoretical yield of $\mathrm{Cl}_{2}$, and percent yield for the reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
06:08

Problem 65

Lead ions can be precipitated from solution with $\mathrm{NaCl}$ according to the reaction:
$$\mathrm{Pb}^{2+}(a q)+2 \mathrm{NaCl}(a q) \longrightarrow \mathrm{PbCl}_{2}(s)+2 \mathrm{Na}^{+}(a q)$$
When $135.8 \mathrm{g}$ of $\mathrm{NaCl}$ are added to a solution containing $195.7 \mathrm{g}$ of $\mathrm{Pb}^{2+}, \mathrm{a} \mathrm{PbCl}_{2}$ precipitate forms. The precipitate is filtered and dried and found to have a mass of $252.4 \mathrm{g}$. Determine the limiting reactant, theoretical yield of $\mathrm{PbCl}_{2}$, and percent yield for the reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:42

Problem 66

Magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: $$2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MgO}(s)$$
When $10.1 \mathrm{g}$ of $\mathrm{Mg}$ react with $10.5 \mathrm{g}$ of $\mathrm{O}_{2}, 11.9 \mathrm{g}$ of $\mathrm{MgO}$ are collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:55

Problem 67

Consider the reaction between $\mathrm{TiO}_{2}$ and $\mathrm{C}$ :
$$\mathrm{TiO}_{2}(s)+2 \mathrm{C}(s) \longrightarrow \mathrm{Ti}(s)+2 \mathrm{CO}(g)$$
A reaction vessel initially contains $10.0 \mathrm{g}$ of each of the reactants. Calculate the masses of $\mathrm{Ti} \mathrm{O}_{2}, \mathrm{C}, \mathrm{Ti},$ and $\mathrm{CO}$ that will be in the reaction vessel after the reactants have reacted as much as possible. (Assume $100 \%$ yield.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
06:46

Problem 68

Consider the reaction between $\mathrm{N}_{2} \mathrm{H}_{4}$ and $\mathrm{N}_{2} \mathrm{O}_{4}$ :
$$2 \mathrm{N}_{2} \mathrm{H}_{4}(g)+\mathrm{N}_{2} \mathrm{O}_{4}(g) \longrightarrow 3 \mathrm{N}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$$
A reaction vessel initially contains $27.5 \mathrm{g} \mathrm{N}_{2} \mathrm{H}_{4}$ and $74.9 \mathrm{g}$ of $\mathrm{N}_{2} \mathrm{O}_{4}$. Calculate the masses of $\mathrm{N}_{2} \mathrm{H}_{4}, \mathrm{N}_{2} \mathrm{O}_{4}, \mathrm{N}_{2},$ and $\mathrm{H}_{2} \mathrm{O}$
that will be in the reaction vessel after the reactants have reacted as much as possible. (Assume $100 \%$ yield.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:02

Problem 69

Classify each process as exothermic or endothermic and indicate the sign of $\Delta H_{\mathrm{rxn}}$.
(a) butane gas burning in a lighter
(b) the reaction that occurs in the chemical cold packs used to ice athletic injuries
(c) the burning of wax in a candle

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:21

Problem 70

Classify each process as exothermic or endothermic and indicate the sign of $\Delta H_{\mathrm{rxn}}$.
(a) ice melting
(b) a sparkler burning
(c) acetone evaporating from skin

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:58

Problem 71

Consider the generic reaction:
$$\mathrm{A}+2 \mathrm{B} \longrightarrow \mathrm{C} \quad \Delta H_{\mathrm{rxn}}=-55 \mathrm{kJ}$$
Determine the amount of heat emitted when each amount of reactant completely reacts (assume that there is more than enough of the other reactant).
(a) $1 \mathrm{mol} \mathrm{A}$
(b) $2 \mathrm{mol} \mathrm{A}$
(c) $1 \mathrm{mol} \mathrm{B}$
(d) $2 \mathrm{mol} \mathrm{B}$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:53

Problem 72

Consider the generic reaction:
$$2 \mathrm{A}+3 \mathrm{B} \longrightarrow \mathrm{C} \quad \Delta H_{\mathrm{rxn}}=-125 \mathrm{kJ}$$
Determine the amount of heat emitted when each amount of reactant completely reacts (assume that there is more than enough of the other reactant).
(a) 2 mol $A$
(b) 3 mol $A$
(c) 3 mol $B$
(d) 5 mol $B$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:26

Problem 73

Consider the equation for the combustion of acetone $\left(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\right),$ the main ingredient in nail polish remover:
$$\begin{aligned}\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l)+4 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(g) & \\\Delta H_{\mathrm{rxn}} &=-1790 \mathrm{kJ}\end{aligned}$$
If a bottle of nail polish remover contains $155 \mathrm{g}$ of acetone, how much heat is released by its complete combustion?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:36

Problem 74

The equation for the combustion of $\mathrm{CH}_{4}$ (the main component of natural gas) is shown below. How much heat is produced by the complete combustion of $237 \mathrm{g}$ of $\mathrm{CH}_{4} ?$
$$\begin{array}{r}\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) \\&\Delta H_{\mathrm{rxn}}=-802.3 \mathrm{kJ} \end{array}$$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:45

Problem 75

Octane $\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)$ is a component of gasoline that burns according to the equation:
$$\begin{aligned}\mathrm{C}_{8} \mathrm{H}_{18}(l)+\frac{25}{2} \mathrm{O}_{2}(g) \longrightarrow 8 \mathrm{CO}_{2}(g)+& 9 \mathrm{H}_{2} \mathrm{O}(g) \\\Delta H_{\mathrm{rxn}}=&-5074.1 \mathrm{kJ}\end{aligned}$$
What mass of octane (in g) is required to produce $1.55 \times 10^{3} \mathrm{kJ}$ of heat?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:22

Problem 76

The evaporation of water is endothermic:
$$\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{O}(g) \quad \Delta H_{\mathrm{rxn}}=+44.01 \mathrm{kJ}$$
What minimum mass of water (in g) has to evaporate to absorb 175 kJ of heat?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:50

Problem 77

Consider the reaction:
$$2 \mathrm{N}_{2}(g)+5 \mathrm{O}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) \longrightarrow 4 \mathrm{HNO}_{3}(g)$$
If a reaction mixture contains $28 \mathrm{g}$ of $\mathrm{N}_{2}, 150 \mathrm{g}$ of $\mathrm{O}_{2},$ and 36 $\mathrm{g}$ of $\mathrm{H}_{2} \mathrm{O},$ what is the limiting reactant? (Try to do this problem in your head without any written calculations.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
01:43

Problem 78

Consider the reaction:
$$2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)$$
If a reaction mixture contains $28 \mathrm{g}$ of $\mathrm{CO}$ and $32 \mathrm{g}$ of $\mathrm{O}_{2}$ what is the limiting reactant? (Try to do this problem in your head without any written calculations.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:45

Problem 79

A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered and dried and found to have a mass of $258 \mathrm{mg}$. What mass of barium was in the original solution? (Assume that all of the barium was precipitated out of solution by the reaction.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:29

Problem 80

A solution contains an unknown mass of dissolved silver ions. When potassium chloride is added to the solution, a white precipitate forms. The precipitate is filtered and dried and found to have a mass of 212 mg. What mass of silver was in the original solution? (Assume that all of the silver was precipitated out of solution by the reaction.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:44

Problem 81

Sodium bicarbonate is often used as an antacid to neutralize excess hydrochloric acid in an upset stomach. How much hydrochloric acid in grams can be neutralized by 3.5 g of sodium bicarbonate? (Hint: Begin by writing a balanced equation for the reaction between aqueous sodium bicarbonate and aqueous hydrochloric acid.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:47

Problem 82

Toilet bowl cleaners often contain hydrochloric acid to dissolve the calcium carbonate deposits that accumulate within a toilet bowl. How much calcium carbonate in grams can be dissolved by $5.8 \mathrm{g}$ of $\mathrm{HCl}$ ? (Hint: Begin by writing a balanced equation for the reaction between hydrochloric acid and calcium carbonate.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:14

Problem 83

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane $\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)$ and calculate how many kilograms of carbon dioxide are added to the atmosphere per $1.0 \mathrm{kg}$ of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:57

Problem 84

Many home barbecues are fueled with propane gas $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ How much carbon dioxide in kilograms is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5 -gal tank)? Assume that the density of the liquid propane in the tank is $0.621 \mathrm{g} / \mathrm{mL}$. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Hailey Tomashek
Hailey Tomashek
Numerade Educator
View

Problem 85

A hard water solution contains $4.8 \mathrm{g}$ of calcium chloride. How much sodium phosphate in grams should be added to the solution to completely precipitate all of the calcium?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:28

Problem 86

Magnesium ions can be precipitated from seawater by the addition of sodium hydroxide. How much sodium hydroxide in grams must be added to a sample of seawater to completely precipitate the $88.4 \mathrm{mg}$ of magnesium present?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:32

Problem 87

Hydrogen gas can be prepared in the laboratory by a single-displacement reaction in which solid zinc reacts with hydrochloric acid. How much zinc in grams is required to make $14.5 \mathrm{g}$ of hydrogen gas through this reaction?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:17

Problem 88

Sodium peroxide $\left(\mathrm{Na}_{2} \mathrm{O}_{2}\right)$ reacts with water to form sodium hydroxide and oxygen gas. Write a balanced equation for the reaction and determine how much oxygen in grams is formed by the complete reaction of $35.23 \mathrm{g}$ of $\mathrm{Na}_{2} \mathrm{O}_{2}$.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:21

Problem 89

Ammonium nitrate reacts explosively upon heating to form nitrogen gas, oxygen gas, and gaseous water. Write a balanced equation for this reaction and determine how much oxygen in grams is produced by the complete reaction of $1.00 \mathrm{kg}$ of ammonium nitrate.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:16

Problem 90

Pure oxygen gas can be prepared in the laboratory by the decomposition of solid potassium chlorate to form solid potassium chloride and oxygen gas. How much oxygen gas in grams can be prepared from $45.8 \mathrm{g}$ of potassium chlorate?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
08:24

Problem 91

Aspirin can be made in the laboratory by reacting acetic anhydride $\left(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}\right)$ with salicylic acid $\left(\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}\right)$ to form aspirin $\left(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\right)$ and acetic acid $\left(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\right) .$ The balanced equation is:
$$\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}+\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3} \longrightarrow \mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}+\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}$$
In a laboratory synthesis, a student begins with $5.00 \mathrm{mL}$ of acetic anhydride (density $=1.08 \mathrm{g} / \mathrm{mL}$ ) and $2.08 \mathrm{g}$ of salicylic acid. Once the reaction is complete, the student collects $2.01 \mathrm{g}$ of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yield for the reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
07:46

Problem 92

The combustion of liquid ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)$ produces carbon dioxide and water. After $3.8 \mathrm{mL}$ of ethanol (density $=0.789 \mathrm{g} / \mathrm{mL}$ ) is allowed to burn in the presence of $12.5 \mathrm{g}$ of oxygen gas, $3.10 \mathrm{mL}$ of water (density $=1.00 \mathrm{g} / \mathrm{mL}$ ) is collected. Determine the limiting reactant, theoretical yield of $\mathrm{H}_{2} \mathrm{O},$ and percent yield for the reaction. (Hint: Write a balanced equation for the combustion of ethanol.)

Zubair Abdulla
Zubair Abdulla
Numerade Educator
06:49

Problem 93

Urea $\left(\mathrm{CH}_{4} \mathrm{N}_{2} \mathrm{O}\right),$ a common fertilizer, can be synthesized by the reaction of ammonia $\left(\mathrm{NH}_{3}\right)$ with carbon dioxide:
$$2 \mathrm{NH}_{3}(a q)+\mathrm{CO}_{2}(a q) \longrightarrow \mathrm{CH}_{4} \mathrm{N}_{2} \mathrm{O}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$$
An industrial synthesis of urea produces $87.5 \mathrm{kg}$ of urea upon reaction of $68.2 \mathrm{kg}$ of ammonia with $105 \mathrm{kg}$ of carbon dioxide. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
07:23

Problem 94

Silicon, which occurs in nature as $\mathrm{SiO}_{2}$, is the material from which most computer chips are made. If $\mathrm{SiO}_{2}$ is heated until it melts into a liquid, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, $52.8 \mathrm{kg}$ of $\mathrm{SiO}_{2}$ reacts with 25.8 kg of carbon to produce 22.4 kg of silicon. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
06:14

Problem 95

The ingestion of lead from food, water, or other environmental sources can cause lead poisoning, a serious condition that affects the central nervous system, causing symptoms such as distractibility, lethargy, and loss of motor function. Lead poisoning is treated with chelating agents, substances that bind to lead and allow it to be eliminated in the urine. A modern chelating agent used for this purpose is succimer $\left(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{4} \mathrm{S}_{2}\right) .$ Suppose you are trying to determine the appropriate dose for succimer treatment of lead poisoning. Assume that a patient's blood lead levels are $0.550 \mathrm{mg} / \mathrm{L}$ that total blood volume is $5.0 \mathrm{L}$, and that $1 \mathrm{mol}$ of succimer binds 1 mol of lead. What minimum mass of succimer in milligrams is needed to bind all of the lead in this patient's bloodstream?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:27

Problem 96

An emergency breathing apparatus placed in mines or caves works via the chemical reaction:
$$4 \mathrm{KO}_{2}(s)+2 \mathrm{CO}_{2}(g) \longrightarrow 2 \mathrm{K}_{2} \mathrm{CO}_{3}(s)+3 \mathrm{O}_{2}(g)$$
If the oxygen supply becomes limited or if the air becomes poisoned, a worker can use the apparatus to breathe while exiting the mine. Notice that the reaction produces $\mathrm{O}_{2}$ which can be breathed, and absorbs $\mathrm{CO}_{2}$, a product of respiration. What minimum amount of $\mathrm{KO}_{2}$ is required for the apparatus to produce enough oxygen to allow the user 15 minutes to exit the mine in an emergency? Assume that an adult consumes approximately 4.4 g of oxygen in 15 minutes of normal breathing.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
06:22

Problem 97

The propane fuel $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ used in gas barbecues burns according to the equation:
$$\begin{array}{r}\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g) \\\Delta H_{\mathrm{rxn}}=-2044 \mathrm{kJ}
\end{array}$$
If a pork roast must absorb $1.6 \times 10^{3} \mathrm{kJ}$ to fully cook, and if only $10 \%$ of the heat produced by the barbecue is actually absorbed by the roast, what mass of $\mathrm{CO}_{2}$ is emitted into the atmosphere during the grilling of the pork roast?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:28

Problem 98

Charcoal is primarily carbon. Determine the mass of $\mathrm{CO}_{2}$ produced by burning enough carbon to produce $5.00 \times 10^{2} \mathrm{kJ}$ of heat.
$$\mathrm{C}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g) \quad \Delta H_{\mathrm{rxn}}=-393.5 \mathrm{kJ}$$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:57

Problem 99

A loud classroom demonstration involves igniting a hydrogen-filled balloon. The hydrogen within the balloon reacts explosively with oxygen in the air to form water according to this reaction:
$$2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)$$
If the balloon is filled with a mixture of hydrogen and oxygen, the explosion is even louder than if the balloon is filled with only hydrogen; the intensity of the explosion depends on the relative amounts of oxygen and hydrogen within the balloon. Consider the molecular views representing different amounts of hydrogen and oxygen in four different balloons. Based on the balanced chemical equation, which balloon will make the loudest explosion?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
03:05

Problem 100

A hydrochloric acid solution will neutralize a sodium hydroxide solution. Consider the molecular views showing one beaker of HCl and four beakers of NaOH. Which NaOH beaker will just neutralize the HCl beaker? Begin by writing a balanced chemical equation for the neutralization reaction.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:12

Problem 101

As we have seen, scientists have grown progressively more worried about the potential for climate change caused by increasing atmospheric carbon dioxide levels. The world burns the fossil fuel equivalent of approximately $9.0 \times 10^{12} \mathrm{kg}$ of petroleum per year. Assume that all of this petroleum is in the form of octane $\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)$ and calculate how much $\mathrm{CO}_{2}$ in kilograms is produced by world fossil fuel combustion per year. (Hint: Begin by writing a balanced equation for the combustion of octane.) If the atmosphere currently contains approximately $3.0 \times 10^{15} \mathrm{kg}$ of $\mathrm{CO}_{2},$ how long will it take for the world's fossil fuel combustion to double the amount of atmospheric carbon dioxide?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
04:13

Problem 102

Lakes that have been acidified by acid rain can be neutralized by the addition of limestone $\left(\mathrm{CaCO}_{3}\right) .$ How much limestone in kilograms would be required to completely neutralize a $5.2 \times 10^{9}-\mathrm{L}$ lake containing $5.0 \times 10^{-3} \mathrm{g}$ of $\mathrm{H}_{2} \mathrm{SO}_{4}$ per liter?

Zubair Abdulla
Zubair Abdulla
Numerade Educator
06:14

Problem 103

What volume of air is needed to burn an entire $55-\mathrm{L}$ (approximately 15-gal) tank of gasoline? Assume that the gasoline is pure octane, $\mathrm{C}_{8} \mathrm{H}_{18}$. Hint: Air is $20 \%$ oxygen, 1 mol of a gas occupies about 25 L at room temperature, and the density of octane is $0.70 \mathrm{g} / \mathrm{cm}^{3}$.

Zubair Abdulla
Zubair Abdulla
Numerade Educator
02:11

Problem 104

Have each member of your group choose a precipitation reaction from Chapter 7 and write a limiting reagent problem based on it. Provide the masses of reactants and the product. Trade problems within your group and solve them by determining the limiting reagent, the theoretical yield, and the percent yield.

David Collins
David Collins
Numerade Educator
04:38

Problem 105

Consider the combustion of propane:
$$\mathrm{C}_{3} \mathrm{H}_{8}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$$
(a) Balance the reaction.
(b) Divide all coefficients by the coefficient on propane, so that you have the reaction for the combustion of 1 mole of propane.
(c) $\Delta H_{\mathrm{rxn}}$ for the combustion of one mole of propane is -2219 kJ. What mass of propane would you need to burn to generate $5.0 \mathrm{MJ}$ of heat?
(d) If propane costs about $0.67 \text{dollars}/ \mathrm{L}$ and has a density of $2.01 \mathrm{g} / \mathrm{cm}^{3}$ how much would it cost to generate $5.0 \mathrm{MJ}$ of heat by burning propane?

Mena Botros
Mena Botros
Numerade Educator