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Introduction to Chemistry

Bishop

Chapter 4

An Introduction to Chemical Reactions - all with Video Answers

Educators

Chapter Questions

00:45

Problem 1

Write the formulas for all of the diatomic elements.

Emily Himsel
Emily Himsel
Numerade Educator
01:07

Problem 2

Predict whether atoms of each of the following pairs of elements would be expected to form ionic or covalent bonds.
a. $\mathrm{Mg}$ and F
b. O and H
c. Fe and O
d. N and Cl

David Collins
David Collins
Numerade Educator
02:03

Problem 3

Describe the structure of liquid water, including a description of water molecules and the attractions between them.

Shazia Naz
Shazia Naz
Numerade Educator
00:41

Problem 4

Write formulas that correspond to the following names.
a. ammonia
b. methane
c. propane
d. water

Nicole Smina
Nicole Smina
Numerade Educator
03:23

Problem 5

Write formulas that correspond to the following names.
a. nitrogen dioxide
b. carbon tetrabromide
c. dibromine monoxide
d. nitrogen monoxide

Pronoy Sinha
Pronoy Sinha
Numerade Educator
03:48

Problem 6

Write formulas that correspond to the following names.
a. lithium fluoride
b. lead(II) hydroxide
c. potassium oxide
d. sodium carbonate
e. chromium(III) chloride
f. sodium hydrogen phosphate

Shahina -
Shahina -
Numerade Educator

Problem 7

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

A chemical change or chemical reaction is a process in which one or more pure substances are _____________ one or more different pure substances.

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Problem 8

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

In chemical reactions, atoms are rearranged and regrouped through the breaking and making of _____________.

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Problem 9

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

A chemical equation is a(n) _____________ of a chemical reaction.

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Problem 10

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

If special conditions are necessary for a reaction to take place, they are often specified _____________ the arrow in the reaction’s chemical equation.

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Problem 11

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

To indicate that a chemical reaction requires the _____________ addition of heat in order to proceed, we place an upper-case Greek _____________ above the arrow in the reaction’s chemical equation.

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Problem 12

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

In chemical reactions, atoms are neither _____________ nor _____________; they merely change partners. Thus the number of atoms of an element in the reaction’s products is _____________ the number of atoms of that element in the original reactants. The _____________ we often place in front of one or more of the formulas in a chemical equation reflect this fact.

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Problem 13

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

When balancing chemical equations, we do not change the _____________ in the formulas.

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Problem 14

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

A solution, also called a(n) _____________, is a mixture whose particles are so evenly distributed that the relative concentrations of the components are the same throughout.

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Problem 15

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

Every part of a water solution of an ionic compound has the _____________ of water molecules and ions as every other part.

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Problem 16

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

When an ionic compound dissolves in water, the ions that escape the solid are held in solution by attractions between their own _____________ and the _____________ of the polar water molecules. The _____________ oxygen ends of the water molecules surround the cations, and the _____________ hydrogen ends surround the anions.

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Problem 17

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

In solutions of solids dissolved in liquids, we call the solid the _____________ and the liquid the _____________.

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Problem 18

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

In solutions of gases in liquids, we call the _____________ the solute and the _____________ the solvent.

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Problem 19

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

In solutions of two liquids, we call the _____________ component the solute and the _____________ component the solvent.

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Problem 20

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

Sometimes a double-displacement reaction has one product that is insoluble in water. As that product forms, it emerges, or _____________, from the solution as a solid. This process is called _____________, and the solid is called a(n) _____________.

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Problem 21

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

Crystals are solid particles whose component atoms, ions, or molecules are arranged in a(n) _____________ pattern.

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Problem 22

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

In a complete ionic equation, which describes the forms taken by the various substances in solution, the ionic compounds dissolved in the water are described as _____________, and the insoluble ionic compound is described with a(n) _____________.

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Problem 23

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

Because spectator ions are not involved in the reaction, they are often _____________ of the chemical equation.

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Problem 24

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { above } & \text { minor } \\
\text { charge } & \text { negative } \\
\text { chemical bonds } & \text { none } \\
\text { coefficients } & \text { organized, repeating } \\
\text { complete formula } & \text { partial charges } \\
\text { continuous } & \text { positive } \\
\text { converted into } & \text { precipitate } \\
\text { created } & \text { precipitates } \\
\text { delta, } \Delta & \text { precipitation } \\
\text { destroyed } & \text { same proportions } \\
\text { equal to } & \text { separate ions } \\
\text { gas } & \text { shorthand description } \\
\text { homogeneous mixture } & \text { solute } \\
\text { left out } & \text { solvent } \\
\text { liquid } & \text { subscripts } \\
\text { major } & \text { very low }
\end{array}
$$

When we say an ionic solid is insoluble in water, we do not mean that _____________ of the solid dissolves. Thus, when we say that calcium carbonate is insoluble in water, what we really mean is that the solubility is _____________.

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01:55

Problem 25

Describe the information given in the following chemical equation.

$$
2 \mathrm{CuHCO}_3(\mathrm{~s}) \xrightarrow{\Delta} \mathrm{Cu}_2 \mathrm{CO}_3(\mathrm{~s})+\mathrm{H}_2 \mathrm{O}(l)+\mathrm{CO}_2(\mathrm{~g})
$$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
01:58

Problem 26

Describe the information given in the following chemical equation.

$$
2 \mathrm{NaCl}(l) \xrightarrow{\text { Electric current }} 2 \mathrm{Na}(s)+\mathrm{Cl}_2(\mathrm{~g})
$$

Lottie Adams
Lottie Adams
Numerade Educator
06:19

Problem 27

Balance the following equations.
a. $\mathrm{N}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g}) \rightarrow \mathrm{NH}_3(\mathrm{~g})$
$\mathrm{NH}_3$ is used to make explosives and rocket fuel.
b. $\mathrm{Cl}_2(\mathrm{~g})+\mathrm{CH}_4(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{HCl}(\mathrm{g})+\mathrm{CO}(\mathrm{g})$

HCl is used to make vinyl chloride, which is then used to make polyvinyl chloride (PVC) plastic.
c. $\mathrm{B}_2 \mathrm{O}_3(s)+\mathrm{NaOH}(a q) \rightarrow \mathrm{Na}_3 \mathrm{BO}_3(a q)+\mathrm{H}_2 \mathrm{O}(l)$
$\mathrm{Na}_3 \mathrm{BO}_3$ is used as an analytical reagent.
d. $\mathrm{Al}(\mathrm{s})+\mathrm{H}_3 \mathrm{PO}_4(a q) \rightarrow \quad \mathrm{AlPO}_4(s)+\mathrm{H}_2(\mathrm{~g})$
$\mathrm{AlPO}_4$ is used in dental cements.
e. $\mathrm{CO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})$

This reaction takes place in the catalytic converter of your car.
f. $\mathrm{C}_6 \mathrm{H}_{14}(l)+\mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(l)$

This is one of the chemical reactions that take place when gasoline is burned.
g. $\mathrm{Sb}_2 \mathrm{~S}_3(\mathrm{~s})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{Sb}_2 \mathrm{O}_3(\mathrm{~s})+\mathrm{SO}_2(\mathrm{~g})$
$\mathrm{Sb}_2 \mathrm{O}_3$ is used to flameproof cloth.
h. $\mathrm{Al}(s)+\mathrm{CuSO}_4(a q) \rightarrow \mathrm{Al}_2\left(\mathrm{SO}_4\right)_3(a q)+\mathrm{Cu}(s)$
$\mathrm{Al}_2\left(\mathrm{SO}_4\right)_3$ has been used in paper production.
i. $\mathrm{P}_2 \mathrm{H}_4(l) \rightarrow \mathrm{PH}_3(g)+\mathrm{P}_4(s)$
$\mathrm{PH}_3$ is use to make semiconductors, and $\mathrm{P}_4$ is used to manufacture phosphoric acid.

Oluwapelumi Kolawole
Oluwapelumi Kolawole
Numerade Educator
04:40

Problem 28

Balance the following equations.
a. $\mathrm{Fe}_2 \mathrm{O}_3(s)+\mathrm{H}_2(g) \rightarrow \mathrm{Fe}(s)+\mathrm{H}_2 \mathrm{O}(l)$

Fe is the primary component in steel.
b. $\mathrm{SCl}_2(l)+\mathrm{NaF}(s) \rightarrow \mathrm{S}_2 \mathrm{Cl}_2(l)+\mathrm{SF}_4(g)+\mathrm{NaCl}(s)$
$\mathrm{S}_2 \mathrm{Cl}_2$ is used to purify sugar juices.
c. $\mathrm{PCl}_5(s)+\mathrm{H}_2 \mathrm{O}(l) \rightarrow \mathrm{H}_3 \mathrm{PO}_4(a q)+\mathrm{HCl}(a q)$
$\mathrm{H}_3 \mathrm{PO}_4$ is used to make fertilizers, soaps, and detergents.
d. $\mathrm{As}(s)+\mathrm{Cl}_2(g) \rightarrow \mathrm{AsCl}_5(s)$
$\mathrm{AsCl}_5$ is an intermediate in the production of arsenic compounds.
e. $\mathrm{C}_2 \mathrm{H}_5 \mathrm{SH}(l)+\mathrm{O}_2(g) \rightarrow \mathrm{CO}_2(g)+\mathrm{H}_2 \mathrm{O}(l)+\mathrm{SO}_2(g)$
$\mathrm{C}_2 \mathrm{H}_5 \mathrm{SH}$ is added to natural gas to give it an odor. Without it or something like it, you would not know when you have a gas leak.
f. $\mathrm{N}_2 \mathrm{O}_5(g) \rightarrow \mathrm{NO}_2(g)+\mathrm{O}_2(g)$
$\mathrm{NO}_2$ is used in rocket fuels.
g. $\mathrm{Mg}(s)+\mathrm{Cr}\left(\mathrm{NO}_3\right)_3(a q) \rightarrow \mathrm{Mg}\left(\mathrm{NO}_3\right)_2(a q)+\mathrm{Cr}(s)$

Cr is used to make stainless steel.
h. $\mathrm{H}_2 \mathrm{O}(\mathrm{g})+\mathrm{NO}(\mathrm{g}) \rightarrow \mathrm{O}_2(\mathrm{~g})+\mathrm{NH}_3(\mathrm{~g})$
$\mathrm{NH}_3$ is used to make fertilizers.
i. $\mathrm{CCl}_4(l)+\mathrm{SbF}_3(\mathrm{~s}) \rightarrow \mathrm{CCl}_2 \mathrm{~F}_2(\mathrm{~g})+\mathrm{SbCl}_3(\mathrm{~s})$
$\mathrm{CCl}_2 \mathrm{~F}_2$ is a chlorofluorocarbon called CFC-12. Although it has had many uses in the past, its use has diminished greatly due to the damage it can do to our protective ozone layer.

JM
Jana Murdock
Numerade Educator
01:33

Problem 29

Because of its toxicity, carbon tetrachloride is prohibited in products intended for home use, but it is used industrially for a variety of purposes, including the production of chlorofluorocarbons (CFCs). It is made in a three-step process. Balance their equations:

$$
\begin{aligned}
& \mathrm{CS}_2+\mathrm{Cl}_2 \rightarrow \mathrm{~S}_2 \mathrm{Cl}_2+\mathrm{CCl}_4 \\
& \mathrm{CS}_2+\mathrm{S}_2 \mathrm{Cl}_2 \rightarrow \mathrm{~S}_8+\mathrm{CCl}_4 \\
& \mathrm{~S}_8+\mathrm{C} \rightarrow \mathrm{CS}_2
\end{aligned}
$$

Noah Barguez-Arias
Noah Barguez-Arias
Numerade Educator
02:01

Problem 30

Chlorofluorocarbons (CFCs) are compounds that contain carbon, fluorine, and chlorine. Because they destroy ozone that forms a protective shield high in earth's atmosphere, their use is being phased out, but at one time they were widely employed as aerosol propellants and as refrigerants. Balance the following equation that shows how the CFCs dichlorodifluoromethane, $\mathrm{CCl}_2 \mathrm{~F}_2$, and trichlorofluoromethane, $\mathrm{CCl}_3 \mathrm{~F}$, are produced.

$$
\mathrm{HF}+\mathrm{CCl}_4 \rightarrow \mathrm{CCl}_2 \mathrm{~F}_2+\mathrm{CCl}_3 \mathrm{~F}+\mathrm{HCl}
$$

Crystal Wang
Crystal Wang
Numerade Educator
01:23

Problem 31

Hydrochlorofluorocarbons (HCFCs), which contain hydrogen as well as carbon, fluorine, and chlorine, are less damaging to the ozone layer than the chlorofluorocarbons (CFCs) described in problem 30. HCFCs are therefore used instead of CFCs for many purposes. Balance the following equation that shows how the HCFC chlorodifluoromethane, $\mathrm{CHClF}_2$, is made.

$$
\mathrm{HF}+\mathrm{CHCl}_3 \rightarrow \mathrm{CHClF}_2+\mathrm{HCl}
$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
05:40

Problem 32

The primary use of 1,2-dichloroethane, $\mathrm{ClCH}_2 \mathrm{CH}_2 \mathrm{Cl}$, is to make vinyl chloride, which is then converted into polyvinyl chloride (PVC) for many purposes, including plastic pipes. Balance the following equation, which describes the industrial reaction for producing 1,2-dichloroethane.

$$
\mathrm{C}_2 \mathrm{H}_4+\mathrm{HCl}+\mathrm{O}_2 \rightarrow \mathrm{ClCH}_2 \mathrm{CH}_2 \mathrm{Cl}+\mathrm{H}_2 \mathrm{O}
$$

Caroline Basil
Caroline Basil
Numerade Educator
03:38

Problem 33

Describe the process for dissolving the ionic compound lithium iodide, LiI, in water, including the nature of the particles in solution and the attractions between the particles in the solution.

David Collins
David Collins
Numerade Educator
01:24

Problem 34

Describe the process for dissolving the ionic compound potassium nitrate, $\mathrm{KNO}_3$, in water, including the nature of the particles in solution and the attractions between the particles in the solution.

David Collins
David Collins
Numerade Educator
01:57

Problem 35

Describe the process for dissolving the ionic compound sodium sulfate, $\mathrm{Na}_2 \mathrm{SO}_4$, in water. Include mention of the nature of the particles in solution and the attractions between the particles in the solution.

Lottie Adams
Lottie Adams
Numerade Educator
00:58

Problem 36

Describe the process for dissolving the ionic compound calcium chloride, $\mathrm{CaCl}_2$, in water. Include mention of the nature of the particles in solution and the attractions between the particles in the solution.

Shazia Naz
Shazia Naz
Numerade Educator
01:16

Problem 37

Solid camphor and liquid ethanol mix to form a solution. Which of these substances is the solute and which is the solvent?

Will Li
Will Li
Numerade Educator
02:43

Problem 38

Gaseous propane and liquid diethyl ether mix to form a solution. Which of these substances is the solute and which is the solvent?

Eileen Sullivan
Eileen Sullivan
Numerade Educator
01:01

Problem 39

Consider a solution of $10 \%$ liquid acetone and $90 \%$ liquid chloroform. Which of these substances is the solute and which is the solvent?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:36

Problem 40

Black and white photographic film has a thin layer of silver bromide deposited on it. Wherever light strikes the film, silver ions are converted to uncharged silver atoms, creating a dark image on the film. Describe the precipitation reaction that takes place between water solutions of silver nitrate, $\mathrm{AgNO}_3(\mathrm{aq})$, and sodium bromide, $\mathrm{NaBr}(a q)$, to form solid silver bromide, $\operatorname{AgBr}(s)$, and aqueous sodium nitrate, $\mathrm{NaNO}_3(\mathrm{aq})$. Include mention of the nature of the particles in the system before and after the reaction, a description of the cause of the reaction, and a description of the attractions between the particles before and after the reaction.
Figure can't copy

Ronald Prasad
Ronald Prasad
Numerade Educator
07:18

Problem 41

Magnesium carbonate is used as an anti-caking agent in powders and as an antacid. Describe the precipitation reaction that takes place between water solutions of magnesium nitrate, $\mathrm{Mg}\left(\mathrm{NO}_3\right)_2(\mathrm{aq})$, and sodium carbonate, $\mathrm{Na}_2 \mathrm{CO}_3(\mathrm{aq})$, to form solid magnesium carbonate, $\mathrm{MgCO}_3(\mathrm{~s})$, and aqueous sodium nitrate, $\mathrm{NaNO}_3(\mathrm{aq})$. Include mention of the nature of the particles in the system before and after the reaction, a description of the cause of the reaction, and a description of the attractions between the particles before and after the reaction.

Nicholas Mogoi
Nicholas Mogoi
Numerade Educator
04:10

Problem 42

Predict whether each of the following substances is soluble or insoluble in water.
a. $\mathrm{Na}_2 \mathrm{SO}_3$ (used in water treatment)
b. iron(III) acetate (a wood preservative)
c. $\mathrm{CoCO}_3$ (a red pigment)
d. lead(II) chloride (used in the preparation of lead salts)

Md Mohibullah
Md Mohibullah
Auburn University Main Campus
01:30

Problem 43

Predict whether each of the following substances is soluble or insoluble in water.
a. $\mathrm{MgSO}_4$ (fireproofing)
b. barium sulfate (used in paints)
c. $\mathrm{Bi}(\mathrm{OH})_3$ (used in plutonium separation)
d. ammonium sulfite (used in medicine and photography)

Nicole Smina
Nicole Smina
Numerade Educator
01:32

Problem 44

Predict whether each of the following substances is soluble or insoluble in water.
a. zinc phosphate (used in dental cements)
b. $\mathrm{Mn}\left(\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2\right)_2$ (used in cloth dyeing)
c. nickel(II) sulfate (used in nickel plating)
d. AgCl (used in silver plating)
Figure can't copy

David Collins
David Collins
Numerade Educator
02:55

Problem 45

Predict whether each of the following substances is soluble or insoluble in water.
a. copper(II) chloride (used in fireworks and as a fungicide)
b. $\mathrm{PbSO}_4$ (a paint pigment)
c. potassium hydroxide (used in soap manufacture)
d. $\mathrm{NH}_4 \mathrm{~F}$ (used as an antiseptic in brewing)

Lottie Adams
Lottie Adams
Numerade Educator
04:19

Problem 46

For each of the following pairs of formulas, predict whether the substances they represent would react in a precipitation reaction. The products formed in the reactions that take place are used in ceramics, cloud seeding, photography, electroplating, and paper coatings. If there is no reaction, write, "No Reaction." If there is a reaction, write the complete equation for the reaction.
a. $\mathrm{Co}\left(\mathrm{NO}_3\right)_2(\mathrm{aq})+\mathrm{Na}_2 \mathrm{CO}_3(\mathrm{aq})$
b. $\mathrm{KI}(\mathrm{aq})+\mathrm{Pb}\left(\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2\right)_2(\mathrm{aq})$
c. $\mathrm{CuSO}_4(\mathrm{aq})+\mathrm{LiNO}_3(\mathrm{aq})$
d. $\mathrm{Ni}\left(\mathrm{NO}_3\right)_2(a q)+\mathrm{Na}_3 \mathrm{PO}_4(a q)$
e. $\mathrm{K}_2 \mathrm{SO}_4(a q)+\mathrm{Ba}\left(\mathrm{NO}_3\right)_2(a q)$

Lottie Adams
Lottie Adams
Numerade Educator
05:07

Problem 47

For each of the following pairs of formulas, predict whether the substances they represent would react in a precipitation reaction. If there is no reaction, write, "No Reaction." If there is a reaction, write the complete equation for the reaction.
a. $\mathrm{NaCl}(a q)+\mathrm{Pb}\left(\mathrm{NO}_3\right)_2(a q)$
b. $\mathrm{NH}_4 \mathrm{Cl}(a q)+\mathrm{CaSO}_3(a q)$
c. $\mathrm{NaOH}(a q)+\mathrm{Zn}\left(\mathrm{NO}_3\right)_2(a q)$
d. $\mathrm{Pb}\left(\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2\right)_2(\mathrm{aq})+\mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq})$

David Collins
David Collins
Numerade Educator
01:15

Problem 48

Phosphate ions find their way into our water system from the fertilizers dissolved in the runoff from agricultural fields and from detergents that we send down our drains. Some of these phosphate ions can be removed by adding aluminum sulfate to the water and precipitating the phosphate ions as aluminum phosphate. Write the net ionic equation for the reaction that forms the aluminum phosphate.

Lottie Adams
Lottie Adams
Numerade Educator
01:37

Problem 49

The taste of drinking water can be improved by removing impurities from our municipal water by adding substances to the water that precipitate a solid (called a flocculent) that drags down impurities as it settles. One way this is done is to dissolve aluminum sulfate and sodium hydroxide in the water to precipitate aluminum hydroxide. Write the complete equation for this reaction.

Gustavo Aroeira
Gustavo Aroeira
Numerade Educator
01:40

Problem 50

Cadmium hydroxide is used in storage batteries. It is made from the precipitation reaction of cadmium acetate and sodium hydroxide. Write the complete equation for this reaction.

Ronald Prasad
Ronald Prasad
Numerade Educator
04:12

Problem 51

Chromium(III) phosphate is a paint pigment that is made in a precipitation reaction between water solutions of chromium(III) chloride and sodium phosphate. Write the complete equation for this reaction.

Vishal Sharma
Vishal Sharma
Numerade Educator
05:20

Problem 52

Balance the following chemical equations.
a. $\mathrm{SiCl}_4+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{SiO}_2+\mathrm{HCl}$
b. $\mathrm{H}_3 \mathrm{BO}_3 \rightarrow \mathrm{~B}_2 \mathrm{O}_3+\mathrm{H}_2 \mathrm{O}$
c. $\mathrm{I}_2+\mathrm{Cl}_2 \rightarrow \mathrm{ICl}_3$
d. $\mathrm{Al}_2 \mathrm{O}_3+\mathrm{C} \rightarrow \mathrm{Al}+\mathrm{CO}_2$

Nadia Lara
Nadia Lara
Numerade Educator
00:59

Problem 53

Balance the following chemical equations.
a. $\mathrm{HClO}_4+\mathrm{Fe}(\mathrm{OH})_2 \rightarrow \mathrm{Fe}\left(\mathrm{ClO}_4\right)_2+\mathrm{H}_2 \mathrm{O}$
b. $\mathrm{NaClO}_3 \rightarrow \mathrm{NaCl}+\mathrm{O}_2$
c. $\mathrm{Sb}+\mathrm{Cl}_2 \rightarrow \mathrm{SbCl}_3$
d. $\mathrm{CaCN}_2+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{CaCO}_3+\mathrm{NH}_3$

Ronald Prasad
Ronald Prasad
Numerade Educator
02:29

Problem 54

Balance the following chemical equations.
a. $\mathrm{NH}_3+\mathrm{Cl}_2 \rightarrow \mathrm{~N}_2 \mathrm{H}_4+\mathrm{NH}_4 \mathrm{Cl}$
b. $\mathrm{Cu}+\mathrm{AgNO}_3 \rightarrow \mathrm{Cu}\left(\mathrm{NO}_3\right)_2+\mathrm{Ag}$
c. $\mathrm{Sb}_2 \mathrm{~S}_3+\mathrm{HNO}_3 \rightarrow \mathrm{Sb}\left(\mathrm{NO}_3\right)_3+\mathrm{H}_2 \mathrm{~S}$
d. $\mathrm{Al}_2 \mathrm{O}_3+\mathrm{Cl}_2+\mathrm{C} \rightarrow \mathrm{AlCl}_3+\mathrm{CO}$

David Collins
David Collins
Numerade Educator
04:40

Problem 55

Balance the following chemical equations.
a. $\mathrm{AsH}_3 \rightarrow \mathrm{As}+\mathrm{H}_2$
b. $\mathrm{H}_2 \mathrm{~S}+\mathrm{Cl}_2 \rightarrow \mathrm{~S}_8+\mathrm{HCl}$
c. $\mathrm{Co}+\mathrm{O}_2 \rightarrow \mathrm{Co}_2 \mathrm{O}_3$
d. $\mathrm{Na}_2 \mathrm{CO}_3+\mathrm{C} \rightarrow \mathrm{Na}+\mathrm{CO}$

JM
Jana Murdock
Numerade Educator
03:40

Problem 56

Phosphoric acid, $\mathrm{H}_3 \mathrm{PO}_4$, is an important chemical used to make fertilizers, detergents, pharmaceuticals, and many other substances. High purity phosphoric acid is made in a two-step process called the furnace process. Balance its two equations:

$$
\begin{aligned}
& \mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2+\mathrm{SiO}_2+\mathrm{C} \rightarrow \mathrm{P}_4+\mathrm{CO}+\mathrm{CaSiO}_3 \\
& \mathrm{P}_4+\mathrm{O}_2+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{H}_3 \mathrm{PO}_4
\end{aligned}
$$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:40

Problem 57

For most applications, phosphoric acid is produced by the "wet process" (whose results are less pure than those of the furnace process described in problem 56). Balance the following equation that describes the reaction for this process.

$$
\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2+\mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{H}_3 \mathrm{PO}_4+\mathrm{CaSO}_4
$$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:11

Problem 58

Predict whether each of the following substances is soluble or insoluble in water.
a. manganese(II) chloride (used as a dietary supplement)
b. $\mathrm{CdSO}_4$ (used in pigments)
c. copper(II) carbonate (used in fireworks)
d. $\mathrm{Co}(\mathrm{OH})_3$ (used as a catalyst)

Nicole Smina
Nicole Smina
Numerade Educator
01:42

Problem 59

Predict whether each of the following substances is soluble or insoluble in water.
a. copper(II) hydroxide (used as a pigment)
b. $\mathrm{BaBr}_2$ (used to make photographic compounds)
c. silver carbonate (used as a laboratory reagent)
d. $\mathrm{Pb}_3\left(\mathrm{PO}_4\right)_2$ (used as a stabilizing agent in plastics)

Eileen Sullivan
Eileen Sullivan
Numerade Educator
01:17

Problem 60

For each of the following pairs of formulas, predict whether the substances they represent would react to yield a precipitate. (The products formed in the reactions that take place are used to coat steel, as a fire-proofing filler for plastics, in cosmetics, and as a topical antiseptic.) If there is no reaction, write, "No Reaction". If there is a reaction, write the complete equation for the reaction.
a. $\mathrm{NaCl}(a q)+\mathrm{Al}\left(\mathrm{NO}_3\right)_3(a q)$
b. $\mathrm{Ni}\left(\mathrm{NO}_3\right)_2(a q)+\mathrm{NaOH}(a q)$
c. $\mathrm{MnCl}_2(a q)+\mathrm{Na}_3 \mathrm{PO}_4(a q)$
d. $\mathrm{Zn}\left(\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2\right)_2(a q)+\mathrm{Na}_2 \mathrm{CO}_3($ aq $)$

Ronald Prasad
Ronald Prasad
Numerade Educator
07:00

Problem 61

For each of the following pairs of formulas, predict whether the substances they represent would react to yield a precipitate. (The products formed in the reactions that take place are used as a catalyst, as a tanning agent, as a pigment, in fertilizers, as a food additive, and on photographic film.) If there is no reaction, write, "No Reaction". If there is a reaction, write the complete equation for the reaction.
a. $\mathrm{KOH}(a q)+\mathrm{Cr}\left(\mathrm{NO}_3\right)_3(a q)$
b. $\mathrm{Fe}\left(\mathrm{NO}_3\right)_3(a q)+\mathrm{K}_3 \mathrm{PO}_4(a q)$
c. $\mathrm{NaBr}(a q)+\mathrm{AgNO}_3(\mathrm{aq})$
d. $\mathrm{Mg}\left(\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2\right)_2(a q)+\mathrm{NaCl}(a q)$

Evan Schroeder
Evan Schroeder
Numerade Educator
08:14

Problem 62

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Hydrochloric acid is used in the cleaning of metals (called pickling). Hydrogen chloride, used to make hydrochloric acid, is made industrially by combining hydrogen and chlorine. Write a balanced equation, without including states, for this reaction.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:08

Problem 63

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Potassium hydroxide has many uses, including the manufacture of soap. It is made by running an electric current through a water solution of potassium chloride. Both potassium chloride and water are reactants, and the products are potassium hydroxide, hydrogen, and chlorine. Write a balanced equation, without including states, for this reaction.

Vishal Sharma
Vishal Sharma
Numerade Educator
03:10

Problem 64

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Aluminum sulfate, commonly called alum, is used to coat paper made from wood pulp. (It fills in tiny holes in the paper and thus keeps the ink from running.) Alum is made in the reaction of aluminum oxide with sulfuric acid, $\mathrm{H}_2 \mathrm{SO}_4$, which produces aluminum sulfate and water. Write a balanced equation, without including states, for this reaction.

Dylan Gunawardene
Dylan Gunawardene
Numerade Educator
01:46

Problem 65

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Under the right conditions, methanol reacts with oxygen to yield formaldehyde, $\mathrm{CH}_2 \mathrm{O}$, and water. Most of the formaldehyde made in this way is used in the production of other substances, including some important plastics. Formaldehyde, itself now a suspected carcinogen, was once used in insulation foams and in plywood adhesives. Write a balanced equation, without including states, for the reaction that produces formaldehyde from methanol.

Julie Guaglianone
Julie Guaglianone
Numerade Educator
03:08

Problem 66

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Hydrogen fluoride is used to make chlorofluorocarbons (CFCs) and in uranium processing. Calcium fluoride reacts with sulfuric acid, $\mathrm{H}_2 \mathrm{SO}_4$, to form hydrogen fluoride and calcium sulfate. Write a balanced equation, without including states, for this reaction.

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
01:58

Problem 67

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Sodium sulfate, which is used to make detergents and glass, is one product of the reaction of sodium chloride, sulfur dioxide, water, and oxygen. The other product is hydrogen chloride. Write a balanced equation, without including states, for this reaction.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:10

Problem 68

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Sodium hydroxide, which is often called caustic soda, is used to make paper, soaps, and detergents. For many years, it was made from the reaction of sodium carbonate with calcium hydroxide (also called slaked lime). The products are sodium hydroxide and calcium carbonate. Write a balanced equation, without including states, for this reaction.

Lottie Adams
Lottie Adams
Numerade Educator
02:54

Problem 69

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
In the modern process for making sodium hydroxide, an electric current is run through a sodium chloride solution, forming hydrogen and chlorine along with the sodium hydroxide. Both sodium chloride and water are reactants. Write a balanced equation, without including states, for this reaction.

LJ
Lena Jake
Numerade Educator
05:23

Problem 70

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
For over a century, sodium carbonate (often called soda ash) was made industrially by the Solvay process. This process was designed by Ernest Solvay in 1864 and was used in the United States until extensive natural sources of sodium carbonate were found in the 1970 s and 1980 s . Write a balanced equation, without including states, for each step in the process:
a. Calcium carbonate (from limestone) is heated and decomposes into calcium oxide and carbon dioxide.
b. Calcium oxide reacts with water to form calcium hydroxide.
c. Ammonia reacts with water to form ammonium hydroxide.
d. Ammonium hydroxide reacts with carbon dioxide to form ammonium hydrogen carbonate.
e. Ammonium hydrogen carbonate reacts with sodium chloride to form sodium hydrogen carbonate and ammonium chloride.
f. Sodium hydrogen carbonate is heated and decomposes into sodium carbonate, carbon dioxide, and water.
g. Ammonium chloride reacts with calcium hydroxide to form ammonia, calcium chloride, and water.

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
12:16

Problem 71

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
All of the equations for the Solvay process described in problem 70 can be summarized by a single equation, called a net equation, that describes the overall change for the process. This equation shows calcium carbonate reacting with sodium chloride to form sodium carbonate and calcium chloride. Write a balanced equation, without including states, for this net reaction.

Christopher Nilsen
Christopher Nilsen
Numerade Educator
12:44

Problem 72

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Nitric acid, $\mathrm{HNO}_3$, which is used to make fertilizers and explosives, is made industrially in the three steps described below. Write a balanced equation, without including states, for each of these steps.
a. Ammonia reacts with oxygen to form nitrogen monoxide and water.
b. Nitrogen monoxide reacts with oxygen to form nitrogen dioxide.
c. Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide.

Shaelyn Deal
Shaelyn Deal
Numerade Educator
12:44

Problem 73

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
All of the equations for the production of nitric acid described in problem 72 can be summarized in a single equation, called a net equation, that describes the overall change for the complete process. This equation shows ammonia combining with oxygen to yield nitric acid and water. Write a balanced equation, without including states, for this net reaction.

Shaelyn Deal
Shaelyn Deal
Numerade Educator
02:19

Problem 74

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Ammonium sulfate, an important component in fertilizers, is made from the reaction of ammonia and sulfuric acid, $\mathrm{H}_2 \mathrm{SO}_4$. Write a balanced equation, without including states, for the reaction that summarizes this transformation.

Nicholas Mogoi
Nicholas Mogoi
Numerade Educator
03:56

Problem 75

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Hydrogen gas has many practical uses, including the conversion of vegetable oils into margarine. One way the gas is produced by the chemical industry is by reacting propane gas with gaseous water to form carbon dioxide gas and hydrogen gas. Write a balanced equation for this reaction, showing the states of reactants and products.

Daniel Kim
Daniel Kim
Numerade Educator
01:07

Problem 76

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Sodium tripolyphosphate, $\mathrm{Na}_5 \mathrm{P}_3 \mathrm{O}_{10}$, is called a "builder" when added to detergents. It helps to create the conditions in laundry water necessary for the detergents to work most efficiently. When phosphoric acid, $\mathrm{H}_3 \mathrm{PO}_4$, is combined with sodium carbonate, three reactions take place in the mixture that lead to the production of sodium tripolyphosphate. Write a balanced equation, without including states, for each of the reactions:
a. Phosphoric acid reacts with sodium carbonate to form sodium dihydrogen phosphate, water, and carbon dioxide.
b. Phosphoric acid also reacts with sodium carbonate to form sodium hydrogen phosphate, water, and carbon dioxide.
c. Sodium dihydrogen phosphate combines with sodium hydrogen phosphate to yield sodium tripolyphosphate and water.

Mikayla Stephens
Mikayla Stephens
Numerade Educator
09:12

Problem 77

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
Pig iron is iron with about $4.3 \%$ carbon in it. The carbon lowers the metal's melting point and makes it easier to shape. To produce pig iron, iron(III) oxide is combined with carbon and oxygen at high temperature. Three changes then take place to form molten iron with carbon dispersed in it. Write a balanced equation, without including states, for each of these changes:
a. Carbon combines with oxygen to form carbon monoxide.
b. Iron(III) oxide combines with the carbon monoxide to form iron and carbon dioxide.
c. Carbon monoxide changes into carbon (in the molten iron) and carbon dioxide.

Katherine Mccandless
Katherine Mccandless
Numerade Educator
04:04

Problem 78

Before working Chapter Problems 62 through 78, you might want to review the procedures for writing chemical formulas that are described in Chapter 3. Remember that some elements are described with formulas containing subscripts (as in $\mathrm{O}_2$ ).
The United States chemical industry makes more sulfuric acid than any other chemical. One process uses hydrogen sulfide from "sour" natural gas wells or petroleum refineries as a raw material. Write a balanced equation, without including states, for each of the steps leading from hydrogen sulfide to sulfuric acid:
a. Hydrogen sulfide (which could be called dihydrogen monosulfide) combines with oxygen to form sulfur dioxide and water.
b. The sulfur dioxide reacts with more hydrogen sulfide to form sulfur and water. (Sulfur is described as both $S$ and $S_8$ in chemical equations. Use $S$ in this equation).
c. After impurities are removed, the sulfur is reacted with oxygen to form sulfur dioxide.
d. Sulfur dioxide reacts with oxygen to yield sulfur trioxide.
e. Sulfur trioxide and water combine to make sulfuric acid, $\mathrm{H}_2 \mathrm{SO}_4$.

Sam Limsuwannarot
Sam Limsuwannarot
Numerade Educator
03:26

Problem 79

Assume you are given a water solution that contains either sodium ions or aluminum ions. Describe how you could determine which of these is in solution.

Adriano Chikande
Adriano Chikande
Numerade Educator
03:26

Problem 80

Assume that you are given a water solution that contains either nitrate ions or phosphate ions. Describe how you could determine which of these is in solution.

Adriano Chikande
Adriano Chikande
Numerade Educator
04:31

Problem 81

Write a complete, balanced chemical equation for the reaction between water solutions of iron(III) chloride and silver nitrate.

Regina Hays
Regina Hays
Numerade Educator
00:43

Problem 82

Write a complete, balanced chemical equation for the reaction between water solutions of sodium phosphate and copper(II) chloride.

Joshua Speer
Joshua Speer
Numerade Educator
01:24

Problem 83

When the solid amino acid methionine, $\mathrm{C}_5 \mathrm{H}_{11} \mathrm{NSO}_2$, reacts with oxygen gas, the products are carbon dioxide gas, liquid water, sulfur dioxide gas, and nitrogen gas. Write a complete, balanced equation for this reaction.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:29

Problem 84

When the explosive liquid nitroglycerin, $\mathrm{C}_3 \mathrm{H}_5 \mathrm{~N}_3 \mathrm{O}_9$, decomposes, it forms carbon dioxide gas, nitrogen gas, water vapor, and oxygen gas. Write a complete, balanced equation for this reaction.

Christopher Nilsen
Christopher Nilsen
Numerade Educator
03:55

Problem 85

The solubility of calcium carbonate is 0.0014 g of $\mathrm{CaCO}_3$ per 100 mL of water at $25^{\circ} \mathrm{C}$, and the solubility of sodium nitrate is 92.1 grams of $\mathrm{NaNO}_3$ per 100 mL of water at $25^{\circ} \mathrm{C}$. We say that calcium carbonate is insoluble in water, and sodium nitrate, $\mathrm{NaNO}_3$, is soluble.
a. In Section 4.6, the following statement was made: "When we say an ionic solid is insoluble in water, we do not mean that none of the solid dissolves. There are always some ions that can escape from the surface of an ionic solid in water and go into solution. "Discuss the process by which calcium and carbonate ions can escape from the surface of calcium carbonate solid in water and go into solution. You might want to draw a picture to illustrate this process.
b. If the calcium and carbonate ions are constantly going into solution, why doesn't the calcium carbonate solid all dissolve?
c. Why do you think sodium nitrate, $\mathrm{NaNO}_3$, dissolves to a much greater degree than calcium carbonate?
d. Why is there a limit to the solubility of even the "soluble" sodium nitrate?

Susan Hallstrom
Susan Hallstrom
Numerade Educator