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Basic Chemistry

Karen C. Timberlake, William Timberlake

Chapter 9

Chemical Quantities in Reactions - all with Video Answers

Educators

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Chapter Questions

04:48

Problem 1

Calculate the total mass of the reactants and the products for each of the following equations:
a. $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)$
b. $4 \mathrm{P}(s)+5 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{P}_{2} \mathrm{O}_{5}(s)$

Sima Sarker
Sima Sarker
Numerade Educator
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Problem 2

Calculate the total mass of the reactants and the products for each of the following equations:
a. $2 \mathrm{Al}(s)+3 \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{AlCl}_{3}(s)$
b. $4 \mathrm{HCl}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Cl}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$

FE
Fatih Elibol
Numerade Educator
01:18

Problem 3

Write all of the mole-mole factors for each of the following chemical equations:
a. $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)$
b. $4 \mathrm{P}(s)+5 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{P}_{2} \mathrm{O}_{5}(s)$

David Collins
David Collins
Numerade Educator
05:02

Problem 4

Write all of the mole-mole factors for each of the following chemical equations:
a. $2 \mathrm{Al}(s)+3 \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{AlCl}_{3}(s)$
b. $4 \mathrm{HCl}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Cl}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$

Vishal Sharma
Vishal Sharma
Numerade Educator
04:31

Problem 5

For the chemical equations in problem $9.3$, write the problem setup with the correct mole-mole factor needed to find each of the following:
a. moles of $\mathrm{SO}_{3}$ from the moles of $\mathrm{SO}_{2}$
b. moles of $\mathrm{O}_{2}$ needed to react with moles of $\mathrm{P}$

Courtney R
Courtney R
Numerade Educator
02:47

Problem 6

For the chemical equations in problem $9.4$, write the problem setup with the correct mole-mole factor needed to find each of the following:
a. moles of $\mathrm{AlCl}_{3}$ from the moles of $\mathrm{Cl}_{2}$
b. moles of $\mathrm{O}_{2}$ needed to react with moles of $\mathrm{HCl}$

Pam Owens
Pam Owens
Numerade Educator
04:48

Problem 7

The chemical reaction of hydrogen with oxygen produces water.
$$
2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{O}_{2}$ are required to react with $2.6 \mathrm{~mol}$ of $\mathrm{H}_{2}$ ?
b. How many moles of $\mathrm{H}_{2}$ are needed to react with $5.0 \mathrm{~mol}$ of $\mathrm{O}_{2}$ ?
c. How many moles of $\mathrm{H}_{2} \mathrm{O}$ form when $2.5 \mathrm{~mol}$ of $\mathrm{O}_{2}$ reacts?

Courtney R
Courtney R
Numerade Educator
05:43

Problem 8

Ammonia is produced by the chemical reaction of nitrogen and hydrogen.
$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$
a. How many moles of $\mathrm{H}_{2}$ are needed to react with $1.8 \mathrm{~mol}$ of $\mathrm{N}_{2}$ ?
b. How many moles of $\mathrm{N}_{2}$ reacted if $0.60 \mathrm{~mol}$ of $\mathrm{NH}_{3}$ is produced?
c. How many moles of $\mathrm{NH}_{3}$ are produced when $1.4 \mathrm{~mol}$ of $\mathrm{H}_{2}$ reacts?

Courtney R
Courtney R
Numerade Educator
07:36

Problem 9

Carbon disulfide and carbon monoxide are produced when carbon is heated with sulfur dioxide.
$$
5 \mathrm{C}(s)+2 \mathrm{SO}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CS}_{2}(l)+4 \mathrm{CO}(g)
$$
a. How many moles of $\mathrm{C}$ are needed to react with $0.500 \mathrm{~mol}$ of $\mathrm{SO}_{2}$ ?
b. How many moles of $\mathrm{CO}$ are produced when $1.2 \mathrm{~mol}$ of $\mathrm{C}$ reacts?
c. How many moles of $\mathrm{SO}_{2}$ are required to produce $0.50 \mathrm{~mol}$ of $\mathrm{CS}_{2}$ ?
d. How many moles of $\mathrm{CS}_{2}$ are produced when $2.5 \mathrm{~mol}$ of $\mathrm{C}$ reacts?

Courtney R
Courtney R
Numerade Educator
06:54

Problem 10

In the acetylene torch, acetylene gas burns in oxygen to produce carbon dioxide, water, and energy.
$$
2 \mathrm{C}_{2} \mathrm{H}_{2}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)
$$
Acetylene
a. How many moles of $\mathrm{O}_{2}$ are needed to react with $2.40 \mathrm{~mol}$ of $\mathrm{C}_{2} \mathrm{H}_{2}$ ?
b. How many moles of $\mathrm{CO}_{2}$ are produced when $3.5 \mathrm{~mol}$ of $\mathrm{C}_{2} \mathrm{H}_{2}$ reacts?
c. How many moles of $\mathrm{C}_{2} \mathrm{H}_{2}$ are required to produce $0.50 \mathrm{~mol}$ of $\mathrm{H}_{2} \mathrm{O}$ ?
d. How many moles of $\mathrm{CO}_{2}$ are produced when $0.100 \mathrm{~mol}$ of $\mathrm{O}_{2}$ reacts?

Courtney R
Courtney R
Numerade Educator
01:15

Problem 11

Sodium reacts with oxygen to produce sodium oxide.
$$
4 \mathrm{Na}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Na}_{2} \mathrm{O}(s)
$$
a. How many grams of $\mathrm{Na}_{2} \mathrm{O}$ are produced when $57.5 \mathrm{~g}$ of $\mathrm{Na}$ reacts?
b. If you have $18.0 \mathrm{~g}$ of $\mathrm{Na}$, how many grams of $\mathrm{O}_{2}$ are required for reaction?
c. How many grams of $\mathrm{O}_{2}$ are needed in a reaction that produces $75.0 \mathrm{~g}$ of $\mathrm{Na}_{2} \mathrm{O}$ ?

Kratika Bhadauria
Kratika Bhadauria
Numerade Educator
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Problem 12

Nitrogen reacts with hydrogen to produce ammonia.
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)
$$
a. If you have $3.64 \mathrm{~g}$ of $\mathrm{H}_{2}$, how many grams of $\mathrm{NH}_{3}$ can be produced?
b. How many grams of $\mathrm{H}_{2}$ are needed to react with $2.80 \mathrm{~g}$ of $\mathrm{N}_{2}$ ?
c. How many grams of $\mathrm{NH}_{3}$ can be produced from $12.0 \mathrm{~g}$ of $\mathrm{H}_{2}$ ?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
06:54

Problem 13

Ammonia and oxygen react to form nitrogen and water.
$$
4 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many grams of $\mathrm{O}_{2}$ are needed to react with $13.6 \mathrm{~g}$ of $\mathrm{NH}_{3}$ ?
b. How many grams of $\mathrm{N}_{2}$ can be produced when $6.50 \mathrm{~g}$ of $\mathrm{O}_{2}$ reacts?
c. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are formed from the reaction of $34.0 \mathrm{~g}$ of $\mathrm{NH}_{3}$ ?

Ashley Brady
Ashley Brady
Numerade Educator
01:49

Problem 14

Iron(III) oxide reacts with carbon to give iron and carbon monoxide.
$$
\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{C}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}(g)
$$
a. How many grams of $\mathrm{C}$ are required to react with $16.5 \mathrm{~g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ ?
b. How many grams of $\mathrm{CO}$ are produced when $36.0 \mathrm{~g}$ of $\mathrm{C}$ reacts?
c. How many grams of Fe can be produced when $6.00 \mathrm{~g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ reacts?

David Collins
David Collins
Numerade Educator
02:11

Problem 15

Nitrogen dioxide and water react to produce nitric acid, $\mathrm{HNO}_{3}$, and nitrogen oxide.
$$
3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)
$$
a. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are required to react with $28.0 \mathrm{~g}$ of $\mathrm{NO}_{2}$ ?
b. How many grams of $\mathrm{NO}$ are produced from $15.8 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$ ?
c. How many grams of $\mathrm{HNO}_{3}$ are produced from $8.25 \mathrm{~g}$ of $\mathrm{NO}_{2}$ ?

David Collins
David Collins
Numerade Educator
13:37

Problem 16

Calcium cyanamide, $\mathrm{CaCN}_{2}$, reacts with water to form calcium carbonate and ammonia.
$$
\mathrm{CaCN}_{2}(s)+3 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{CaCO}_{3}(s)+2 \mathrm{NH}_{3}(g)
$$
a. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are needed to react with $75.0 \mathrm{~g}$ of $\mathrm{CaCN}_{2}$ ?
b. How many grams of $\mathrm{NH}_{3}$ are produced from $5.24 \mathrm{~g}$ of $\mathrm{CaCN}_{2}$ ?
c. How many grams of $\mathrm{CaCO}_{3}$ form if $155 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$ reacts?

Noah Boudrie
Noah Boudrie
Numerade Educator
04:32

Problem 17

When solid lead(II) sulfide reacts with oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas.
a. Write the balanced chemical equation for the reaction.
b. How many grams of oxygen are required to react with $29.9 \mathrm{~g}$ of lead(II) sulfide?
c. How many grams of sulfur dioxide can be produced when $65.0 \mathrm{~g}$ of lead(II) sulfide reacts?
d. How many grams of lead(II) sulfide are used to produce $128 \mathrm{~g}$ of lead(II) oxide?

David Collins
David Collins
Numerade Educator
05:42

Problem 18

When the gases dihydrogen sulfide and oxygen react, they form the gases sulfur dioxide and water vapor.
a. Write the balanced chemical equation for the reaction.
b. How many grams of oxygen are required to react with $2.50 \mathrm{~g}$ of dihydrogen sulfide?
c. How many grams of sulfur dioxide can be produced when $38.5 \mathrm{~g}$ of oxygen reacts?
d. How many grams of oxygen are required to produce $55.8 \mathrm{~g}$ of water vapor?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:13

Problem 19

A taxi company has 10 taxis.
a. On a certain day, only eight taxi drivers show up for work. How many taxis can be used to pick up passengers?
b. On another day, 10 taxi drivers show up for work but three taxis are in the repair shop. How many taxis can be driven?

Ashley Brady
Ashley Brady
Numerade Educator
01:43

Problem 20

A clock maker has 15 clock faces. Each clock requires one face and two hands.
a. If the clock maker has 42 hands, how many clocks can be produced?
b. If the clock maker has only eight hands, how many clocks can be produced?

Ashley Brady
Ashley Brady
Numerade Educator
06:38

Problem 21

Nitrogen and hydrogen react to form ammonia.
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)
$$
Determine the limiting reactant in each of the following mixtures of reactants:
a. $3.0 \mathrm{~mol}$ of $\mathrm{N}_{2}$ and $5.0 \mathrm{~mol}$ of $\mathrm{H}_{2}$
b. $8.0 \mathrm{~mol}$ of $\mathrm{N}_{2}$ and $4.0 \mathrm{~mol}$ of $\mathrm{H}_{2}$
c. $3.0 \mathrm{~mol}$ of $\mathrm{N}_{2}$ and $12.0 \mathrm{~mol}$ of $\mathrm{H}_{2}$

JF
Jordon Flynn
Numerade Educator
06:09

Problem 22

Iron and oxygen react to form iron(III) oxide.
$$
4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)
$$
Determine the limiting reactant in each of the following mixtures of reactants:
a. $2.0 \mathrm{~mol}$ of $\mathrm{Fe}$ and $6.0 \mathrm{~mol}$ of $\mathrm{O}_{2}$
b. $5.0 \mathrm{~mol}$ of $\mathrm{Fe}$ and $4.0 \mathrm{~mol}$ of $\mathrm{O}_{2}$
c. $16.0 \mathrm{~mol}$ of $\mathrm{Fe}$ and $20.0 \mathrm{~mol}$ of $\mathrm{O}_{2}$

JF
Jordon Flynn
Numerade Educator
18:59

Problem 23

For each of the following reactions, $20.0 \mathrm{~g}$ of each reactant is present initially. Determine the limiting reactant, and calculate the grams of product in parentheses that would be produced.
a. $2 \mathrm{Al}(s)+3 \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{AlCl}_{3}(s) \quad\left(\mathrm{AlCl}_{3}\right)$
b. $4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \quad\left(\mathrm{H}_{2} \mathrm{O}\right)$
c. $\mathrm{CS}_{2}(g)+3 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CO}_{2}(g)+2 \mathrm{SO}_{2}(g)\left(\mathrm{SO}_{2}\right)$

JF
Jordon Flynn
Numerade Educator
16:21

Problem 24

For each of the following reactions, $20.0 \mathrm{~g}$ of each reactant is present initially. Determine the limiting reactant, and calculate the grams of product in parentheses that would be produced.
a. $4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(s) \quad\left(\mathrm{Al}_{2} \mathrm{O}_{3}\right)$
b. $3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g) \quad\left(\mathrm{HNO}_{3}\right)$
c. $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}(l)+3 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(g) \quad\left(\mathrm{H}_{2} \mathrm{O}\right)$

JF
Jordon Flynn
Numerade Educator
01:00

Problem 25

For each of the following reactions, calculate the grams of indicated product when $25.0 \mathrm{~g}$ of the first reactant and $40.0 \mathrm{~g}$ of the second reactant are used:
a. $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g) \quad\left(\mathrm{SO}_{3}\right)$
b. $3 \mathrm{Fe}(s)+4 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+4 \mathrm{H}_{2}(g) \quad\left(\mathrm{Fe}_{3} \mathrm{O}_{4}\right)$
c. $\mathrm{C}_{7} \mathrm{H}_{16}(l)+11 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 7 \mathrm{CO}_{2}(g)+8 \mathrm{H}_{2} \mathrm{O}(g) \quad\left(\mathrm{CO}_{2}\right)$

Cheryl Glor
Cheryl Glor
Numerade Educator
View

Problem 26

For each of the following reactions, calculate the grams of indicated product when $15.0 \mathrm{~g}$ of the first reactant and $10.0 \mathrm{~g}$ of the second reactant are used:
a. $4 \mathrm{Li}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Li}_{2} \mathrm{O}(s) \quad\left(\mathrm{Li}_{2} \mathrm{O}\right)$
b. $\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{H}_{2} \mathrm{O}(l)$ (Fe)
c. $\mathrm{Al}_{2} \mathrm{~S}_{3}(s)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{Al}(\mathrm{OH})_{3}(a q)+3 \mathrm{H}_{2} \mathrm{~S}(g) \quad\left(\mathrm{H}_{2} \mathrm{~S}\right)$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
05:01

Problem 27

Carbon disulfide is produced by the reaction of carbon and sulfur dioxide.
$$
5 \mathrm{C}(s)+2 \mathrm{SO}_{2}(g) \longrightarrow \mathrm{CS}_{2}(g)+4 \mathrm{CO}(g)
$$
a. What is the percent yield of carbon disulfide if the reaction of $40.0 \mathrm{~g}$ of carbon produces $36.0 \mathrm{~g}$ of carbon disulfide?
b. What is the percent yield of carbon disulfide if the reaction of $32.0 \mathrm{~g}$ of sulfur dioxide produces $12.0 \mathrm{~g}$ of carbon disulfide?

Ashley Brady
Ashley Brady
Numerade Educator
07:45

Problem 28

Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide.
$$
\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)
$$
a. What is the percent yield of iron if the reaction of $65.0 \mathrm{~g}$ of iron(III) oxide produces $15.0 \mathrm{~g}$ of iron?
b. What is the percent yield of carbon dioxide if the reaction of $75.0 \mathrm{~g}$ of carbon monoxide produces $85.0 \mathrm{~g}$ of carbon dioxide?

Ashley Brady
Ashley Brady
Numerade Educator
02:53

Problem 29

Aluminum reacts with oxygen to produce aluminum oxide.
$$
4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(s)
$$
Calculate the mass of $\mathrm{Al}_{2} \mathrm{O}_{3}$ that can be produced if the reaction of $50.0 \mathrm{~g}$ of aluminum and sufficient oxygen has a $75.0 \%$ yield.

Victoria Moyer
Victoria Moyer
Numerade Educator
View

Problem 30

Propane $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ burns in oxygen to produce carbon dioxide and water.
$$
\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)
$$
Calculate the mass of $\mathrm{CO}_{2}$ that can be produced if the reaction of $45.0 \mathrm{~g}$ of propane and sufficient oxygen has a $60.0 \%$ yield.

Ashley Brady
Ashley Brady
Numerade Educator
04:49

Problem 31

When $30.0 \mathrm{~g}$ of carbon is heated with silicon dioxide, $28.2 \mathrm{~g}$ of carbon monoxide is produced. What is the percent yield of carbon monoxide for this reaction?
$$
\mathrm{SiO}_{2}(s)+3 \mathrm{C}(s) \stackrel{\Delta}{\longrightarrow} \operatorname{SiC}(s)+2 \mathrm{CO}(g)
$$

Courtney R
Courtney R
Numerade Educator
View

Problem 32

When $56.6 \mathrm{~g}$ of calcium is reacted with nitrogen gas, $32.4 \mathrm{~g}$ of calcium nitride is produced. What is the percent yield of calcium nitride for this reaction?
$$
3 \mathrm{Ca}(s)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{Ca}_{3} \mathrm{~N}_{2}(s)
$$

Ashley Brady
Ashley Brady
Numerade Educator
00:39

Problem 33

In an exothermic reaction, is the energy of the products higher or lower than that of the reactants?

Emily Himsel
Emily Himsel
Numerade Educator
00:41

Problem 34

In an endothermic reaction, is the energy of the products higher or lower than that of the reactants?

Emily Himsel
Emily Himsel
Numerade Educator
01:11

Problem 35

Classify each of the following as exothermic or endothermic:
a. A reaction releases $550 \mathrm{~kJ}$.
b. The energy level of the products is higher than that of the reactants.
c. The metabolism of glucose in the body provides energy.

David Collins
David Collins
Numerade Educator
01:26

Problem 36

Classify each of the following as exothermic or endothermic:
a. The energy level of the products is lower than that of the reactants.
b. In the body, the synthesis of proteins requires energy.
c. A reaction absorbs $125 \mathrm{~kJ}$.

David Collins
David Collins
Numerade Educator
01:12

Problem 37

Classify each of the following as exothermic or endothermic, and give the $\Delta H$ for each:
a. $\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)+802 \mathrm{~kJ}$
b. $\mathrm{Ca}(\mathrm{OH})_{2}(s)+65.3 \mathrm{~kJ} \longrightarrow \mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l)$
c. $2 \mathrm{Al}(s)+\mathrm{Fe}_{2} \mathrm{O}_{3}(s) \longrightarrow \mathrm{Al}_{2} \mathrm{O}_{3}(s)+2 \mathrm{Fe}(l)+850 \mathrm{~kJ}$
The thermite reaction of aluminum and iron(III) oxide produces very high temperatures used to cut or weld railroad tracks.

Nicole Smina
Nicole Smina
Numerade Educator
01:10

Problem 38

Classify each of the following as exothermic or endothermic, and give the $\Delta H$ for each:
a. $\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)+2220 \mathrm{~kJ}$
b. $2 \mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NaCl}(s)+819 \mathrm{~kJ}$
c. $\mathrm{PCl}_{5}(g)+67 \mathrm{~kJ} \longrightarrow \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)$

Nicole Smina
Nicole Smina
Numerade Educator
01:35

Problem 39

a. How many kilojoules are released when $125 \mathrm{~g}$ of $\mathrm{Cl}_{2}$ reacts with silicon?
$$
\mathrm{Si}(s)+2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{SiCl}_{4}(g) \quad \Delta H=-657 \mathrm{~kJ}
$$
b. How many kilojoules are absorbed when $278 \mathrm{~g}$ of $\mathrm{PCl}_{5}$ reacts?
$$
\mathrm{PCl}_{5}(g) \longrightarrow \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \quad \Delta H=+67 \mathrm{~kJ}
$$

David Collins
David Collins
Numerade Educator
04:23

Problem 40

a. How many kilojoules are released when $75.0 \mathrm{~g}$ of $\mathrm{CH}_{4} \mathrm{O}$ reacts?
$2 \mathrm{CH}_{4} \mathrm{O}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)$
$\Delta H=-726 \mathrm{~kJ}$
b. How many kilojoules are absorbed when $315 \mathrm{~g}$ of $\mathrm{Ca}(\mathrm{OH})_{2}$ reacts?
$$
\mathrm{Ca}(\mathrm{OH})_{2}(s) \longrightarrow \mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \quad \Delta H=+65.3 \mathrm{~kJ}
$$

Dennis Howard
Dennis Howard
Numerade Educator
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Problem 41

Calculate the energy change for the reaction
$$
\begin{array}{ll}
\mathrm{N}_{2}(g)+2 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) \text { from the following: } \\
\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}(g) & \Delta H=+180 \mathrm{~kJ} \\
2 \mathrm{NO}_{2}(g) \longrightarrow 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) & \Delta H=+114 \mathrm{~kJ}
\end{array}
$$

Ronald Prasad
Ronald Prasad
Numerade Educator
06:47

Problem 42

Calculate the energy change for the reaction $\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow 2 \mathrm{FeO}(s)+\mathrm{CO}_{2}(g)$ from the following:
$$
\begin{array}{ll}
\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g) & \Delta H=-23.4 \mathrm{~kJ} \\
\mathrm{FeO}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g) & \Delta H=-10.9 \mathrm{~kJ}
\end{array}
$$

Catherine Lemar
Catherine Lemar
Numerade Educator
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Problem 43

Calculate the energy change for the reaction $\mathrm{S}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{SO}_{2}(g)$ from the following:
$$
\begin{array}{ll}
2 \mathrm{~S}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g) & \Delta H=-792 \mathrm{~kJ} \\
2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g) & \Delta H=-198 \mathrm{~kJ}
\end{array}
$$

Ronald Prasad
Ronald Prasad
Numerade Educator
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Problem 44

Calculate the energy change for the reaction
$$
\begin{array}{ll}
3 \mathrm{C}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{C}_{3} \mathrm{O}_{2}(g) \text { from the following: } \\
2 \mathrm{CO}(g)+\mathrm{C}(s) \longrightarrow \mathrm{C}_{3} \mathrm{O}_{2}(g) & \Delta H=+127 \mathrm{~kJ} \\
2 \mathrm{C}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}(g) & \Delta H=-222 \mathrm{~kJ}
\end{array}
$$

Ronald Prasad
Ronald Prasad
Numerade Educator
05:34

Problem 45

In one step in the synthesis of the insecticide carbaryl (Sevin), naphthol reacts with phosgene as shown.
$$
\mathrm{C}_{10} \mathrm{H}_{8} \mathrm{O}+\mathrm{COCl}_{2} \longrightarrow \mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}+\mathrm{HCl}
$$
Naphthol Phosgene
a. How many kilograms of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ form from $2.2 \times 10^{2} \mathrm{~kg}$ of naphthol?
b. If $100 . \mathrm{g}$ of naphthol and 100 . g of phosgene react, what is the theoretical yield of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ ?
c. If the actual yield of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ in part b is $115 \mathrm{~g}$, what is the percent yield of $\mathrm{C}_{11} \mathrm{H}_{7} \mathrm{O}_{2} \mathrm{Cl}$ ?

Matthew Kieras
Matthew Kieras
Numerade Educator
05:16

Problem 46

Another widely used insecticide is carbofuran (Furadan), an extremely toxic compound. In one step in the synthesis of carbofuran, the reaction shown is used.
$$
\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{2}+\mathrm{C}_{4} \mathrm{H}_{7} \mathrm{Cl} \longrightarrow \mathrm{C}_{10} \mathrm{H}_{12} \mathrm{O}_{2}+\mathrm{HCl}
$$
a. How many grams of $\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{2}$ are needed to produce $3.8 \times 10^{3} \mathrm{~g}$ of $\mathrm{C}_{10} \mathrm{H}_{12} \mathrm{O}_{2}$ ?
b. If $67.0 \mathrm{~g} \mathrm{of} \mathrm{}_{6} \mathrm{H}_{6} \mathrm{O}_{2}$ and $51.0 \mathrm{~g}$ of $\mathrm{C}_{4} \mathrm{H}_{7} \mathrm{Cl}$ react, what is the theoretical yield of $\mathrm{C}_{10} \mathrm{H}_{12} \mathrm{O}_{2}$ ?
c. If the actual yield of $\mathrm{C}_{10} \mathrm{H}_{12} \mathrm{O}_{2}$ in part b is $85.7 \mathrm{~g}$, what is the percent yield of $\mathrm{C}_{10} \mathrm{H}_{12} \mathrm{O}_{2}$ ?

Matthew Kieras
Matthew Kieras
Numerade Educator
02:51

Problem 47

If red spheres represent oxygen atoms, blue spheres represent nitrogen atoms, and all the molecules are gases, $(9.2,9.4)$
a. write a balanced equation for the reaction.
b. identify the limiting reactant.

Dennis Howard
Dennis Howard
Numerade Educator
04:23

Problem 48

If green spheres represent chlorine atoms, yellow-green spheres represent fluorine atoms, white spheres represent hydrogen atoms, and all the molecules are gases, $(9.2,9.4)$
a. write a balanced equation for the reaction.
b. identify the limiting reactant.

Dennis Howard
Dennis Howard
Numerade Educator
03:17

Problem 49

If blue spheres represent nitrogen atoms, white spheres represent hydrogen atoms, and all the molecules are gases, $(9.2,9.4)$
Reactants
Products
A
a. write a balanced equation for the reaction.
b. identify the diagram that shows the products.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:34

Problem 50

If purple spheres represent iodine atoms, white spheres represent hydrogen atoms, and all the molecules are gases, $(9.2,9.4)$
Reactants
Products
a. write a balanced equation for the reaction.
b. identify the diagram that shows the products.

Dennis Howard
Dennis Howard
Numerade Educator
03:42

Problem 51

If blue spheres represent nitrogen atoms, purple spheres represent iodine atoms, and the reacting molecules are solid, and the products are gases, $(9.2,9.4,9.5)$
a. write a balanced equation for the reaction.
b. from the diagram of the actual products that result, calculate the percent yield for the reaction.

Dennis Howard
Dennis Howard
Numerade Educator
04:54

Problem 52

If green spheres represent chlorine atoms, red spheres represent oxygen atoms, and all the molecules are gases, $(9.2,9.4,9.5)$
a. write a balanced equation for the reaction.
b. identify the limiting reactant.
c. from the diagram of the actual products that result, calculate the percent yield for the reaction.

Dennis Howard
Dennis Howard
Numerade Educator
01:47

Problem 53

Use the balanced chemical equation to complete the table: $(9.1,9.2)$
$$
2 \mathrm{FeS}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{FeO}(s)+2 \mathrm{SO}_{2}(g)
$$
$$
\begin{array}{|l|l|l|l|}
\hline \mathrm{FeS} & \mathrm{O}_{2} & \mathrm{FeO} & \mathrm{SO}_{2} \\
\hline 2.0 \mathrm{~mol} & \mathrm{~mol} & \mathrm{~mol} & \\
\hline & \mathrm{mol} & \mathrm{mol} & \mathrm{mol} \\
\cline { 3 - 4 } & & \mathrm{mol} & 4.6 \mathrm{~mol} \\
\hline
\end{array}
$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:44

Problem 54

Use the balanced chemical equation to complete the table: $(9.1,9.2)$
$$
2 \mathrm{C}_{2} \mathrm{H}_{6}(g)+7 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)
$$
\begin{array}{|r|l|l|l|}
\hline \mathrm{C}_{2} \mathrm{H}_{6} & \mathrm{O}_{2} & \mathrm{CO}_{2} & \mathrm{H}_{2} \mathrm{O} \\
\hline \mathrm{mol} & -\mathrm{mol} & 3.2 \mathrm{~mol} & \mathrm{~mol} \\
\cline { 2 - 4 } \mathrm{mol} & 2.8 \mathrm{~mol} & -\mathrm{mol} & \mathrm{mol} \\
\hline
\end{array}

Aadit Sharma
Aadit Sharma
Numerade Educator
06:16

Problem 55

When ammonia $\left(\mathrm{NH}_{3}\right)$ reacts with fluorine $\left(\mathrm{F}_{2}\right)$, the products are dinitrogen tetrafluoride and hydrogen fluoride. $(9.2,9.3)$
$$
2 \mathrm{NH}_{3}(g)+5 \mathrm{~F}_{2}(g) \longrightarrow \mathrm{N}_{2} \mathrm{~F}_{4}(g)+6 \mathrm{HF}(g)
$$
a. How many moles of each reactant are needed to produce $4.00 \mathrm{~mol}$ of HF?
b. How many grams of $\mathrm{F}_{2}$ are required to react with $25.5 \mathrm{~g}$ of $\mathrm{NH}_{3}$ ?
c. How many grams of $\mathrm{N}_{2} \mathrm{~F}_{4}$ can be produced when $3.40 \mathrm{~g}$ of $\mathrm{NH}_{3}$ reacts?

Matthew Kieras
Matthew Kieras
Numerade Educator
02:01

Problem 56

Gasohol is a fuel that contains ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\right)$ that burns in oxygen $\left(\mathrm{O}_{2}\right)$ to give carbon dioxide and water. $(9.2,9.3)$
$$
\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}(g)+3 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{O}_{2}$ are needed to completely react with $4.0 \mathrm{~mol}$ of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ ?
b. If a car produces $88 \mathrm{~g}$ of $\mathrm{CO}_{2}$, how many grams of $\mathrm{O}_{2}$ are used up in the reaction?
c. If you add $125 \mathrm{~g}$ of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ to your fuel, how many grams of $\mathrm{CO}_{2}$ can be produced from the ethanol?

David Collins
David Collins
Numerade Educator
05:32

Problem 57

When hydrogen peroxide $\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)$ is used in rocket fuels, it produces water and oxygen. $(9.2,9.3)$
$$
2 \mathrm{H}_{2} \mathrm{O}_{2}(l) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)
$$
a. How many moles of $\mathrm{H}_{2} \mathrm{O}_{2}$ are needed to produce $3.00 \mathrm{~mol}$ of $\mathrm{H}_{2} \mathrm{O}$ ?
b. How many grams of $\mathrm{H}_{2} \mathrm{O}_{2}$ are required to produce $36.5 \mathrm{~g}$ of $\mathrm{O}_{2}$ ?
c. How many grams of $\mathrm{H}_{2} \mathrm{O}$ can be produced when $12.2 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}_{2}$ reacts?

Matthew Kieras
Matthew Kieras
Numerade Educator
04:38

Problem 58

Propane gas $\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)$ reacts with oxygen to produce carbon dioxide and water. $(9.2,9.3)$
$$
\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{H}_{2} \mathrm{O}$ form when $5.00 \mathrm{~mol}$ of $\mathrm{C}_{3} \mathrm{H}_{8}$ completely reacts?
b. How many grams of $\mathrm{CO}_{2}$ are produced from $18.5 \mathrm{~g}_{\text {of }} \mathrm{O}_{2}$ ?
c. How many grams of $\mathrm{H}_{2} \mathrm{O}$ can be produced when $46.3 \mathrm{~g}$ of $\mathrm{C}_{3} \mathrm{H}_{8}$ reacts?

Matthew Kieras
Matthew Kieras
Numerade Educator
View

Problem 59

When $12.8 \mathrm{~g}$ of $\mathrm{Na}$ and $10.2 \mathrm{~g}$ of $\mathrm{Cl}_{2}$ react, what is the mass, in grams, of $\mathrm{NaCl}$ that is produced? $(9.2,9.3,9.4)$
$$
2 \mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NaCl}(s)
$$

Lauren Long
Lauren Long
Numerade Educator
04:30

Problem 60

If $35.8 \mathrm{~g}$ of $\mathrm{CH}_{4}$ and $75.5 \mathrm{~g}$ of $\mathrm{S}$ react, how many grams of $\mathrm{H}_{2} \mathrm{~S}$ are produced? $(9.2,9.3,9.4)$
$$
\mathrm{CH}_{4}(g)+4 \mathrm{~S}(g) \longrightarrow \mathrm{CS}_{2}(g)+2 \mathrm{H}_{2} \mathrm{~S}(g)
$$

Heather Gamble
Heather Gamble
Numerade Educator
01:43

Problem 61

Pentane gas $\left(\mathrm{C}_{5} \mathrm{H}_{12}\right)$ reacts with oxygen to produce carbon dioxide and water. $(9.2,9.3,9.4)$
$$
\mathrm{C}_{5} \mathrm{H}_{12}(g)+8 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 5 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{C}_{5} \mathrm{H}_{12}$ must react to produce $4.00 \mathrm{~mol}$ of $\mathrm{H}_{2} \mathrm{O}$ ?
b. How many grams of $\mathrm{CO}_{2}$ are produced from $32.0 \mathrm{~g}$ of $\mathrm{O}_{2}$ ?
c. How many grams of $\mathrm{CO}_{2}$ are formed if $44.5 \mathrm{~g} \mathrm{of} \mathrm{} \mathrm{C}_{5} \mathrm{H}_{12}$ is mixed with $108 \mathrm{~g}$ of $\mathrm{O}_{2}$ ?

David Collins
David Collins
Numerade Educator
04:38

Problem 62

When nitrogen dioxide $\left(\mathrm{NO}_{2}\right)$ from car exhaust combines with water in the air, it forms nitrogen oxide and nitric acid $\left(\mathrm{HNO}_{3}\right)$, which causes acid rain. $(9.2,9.3,9.4)$
$$
3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{NO}(g)+2 \mathrm{HNO}_{3}(a q)
$$
a. How many moles of $\mathrm{NO}_{2}$ are needed to react with $0.250 \mathrm{~mol}$ of $\mathrm{H}_{2} \mathrm{O}$ ?
b. How many grams of $\mathrm{HNO}_{3}$ are produced when $60.0 \mathrm{~g}$ of $\mathrm{NO}_{2}$ completely reacts?
c. How many grams of $\mathrm{HNO}_{3}$ can be produced if $225 \mathrm{~g}$ of $\mathrm{NO}_{2}$ is mixed with $55.2 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$ ?

David Collins
David Collins
Numerade Educator
04:21

Problem 63

The acetylene $\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)$ used in welders' torches, burns according to the following equation: $(9.2,9.3,9.5)$
$$
2 \mathrm{C}_{2} \mathrm{H}_{2}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. What is the theoretical yield, in grams, of $\mathrm{CO}_{2}$, if $22.0 \mathrm{~g}$ of $\mathrm{C}_{2} \mathrm{H}_{2}$ completely reacts?
b. If the actual yield in part a is $64.0 \mathrm{~g}$ of $\mathrm{CO}_{2}$, what is the percent yield of $\mathrm{CO}_{2}$ for the reaction?

Eileen Sullivan
Eileen Sullivan
Numerade Educator
01:57

Problem 64

The equation for the decomposition of potassium chlorate is written as $(9.2,9.3,9.5)$
$$
2 \mathrm{KClO}_{3}(s) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)
$$
a. When $46.0 \mathrm{~g}$ of $\mathrm{KClO}_{3}$ is completely decomposed, what is the theoretical yield, in grams, of $\mathrm{O}_{2}$ ?
b. If the actual yield in part $\mathbf{a}$ is $12.1 \mathrm{~g}$ of $\mathrm{O}_{2}$, what is the percent yield of $\mathrm{O}_{2}$ ?

Adriano Chikande
Adriano Chikande
Numerade Educator
02:24

Problem 65

When $28.0 \mathrm{~g}$ of acetylene reacts with hydrogen, $24.5 \mathrm{~g}$ of ethane is produced. What is the percent yield of $\mathrm{C}_{2} \mathrm{H}_{6}$ for the reaction? $(9.2,9.3,9.5)$
$$
\mathrm{C}_{2} \mathrm{H}_{2}(g)+2 \mathrm{H}_{2}(g) \stackrel{\mathrm{Pt}}{\longrightarrow} \mathrm{C}_{2} \mathrm{H}_{6}(g)
$$

David Collins
David Collins
Numerade Educator
07:45

Problem 66

When $50.0 \mathrm{~g}$ of iron(III) oxide reacts with carbon monoxide, $32.8 \mathrm{~g}$ of iron is produced. What is the percent yield of Fe for the reaction? $(9.2,9.3,9.5)$
$$
\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)
$$

Ashley Brady
Ashley Brady
Numerade Educator
View

Problem 67

Nitrogen and hydrogen combine to form ammonia. $(9.2,9.3$, $9.4,9.5)$
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)
$$
a. If $50.0 \mathrm{~g}$ of $\mathrm{N}_{2}$ is mixed with $20.0 \mathrm{~g}$ of $\mathrm{H}_{2}$, what is the theoretical yield, in grams, of $\mathrm{NH}_{3}$ ?
b. If the reaction in part a has a percent yield of $62.0 \%$, what is the actual yield, in grams, of $\mathrm{NH}_{3}$ ?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:15

Problem 68

Sodium and nitrogen combine to form sodium nitride. $(9.2,9.3$, $9.4,9.5)$
$$
6 \mathrm{Na}(s)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{Na}_{3} \mathrm{~N}(s)
$$
a. If $80.0 \mathrm{~g}$ of $\mathrm{Na}$ is mixed with $20.0 \mathrm{~g}$ of nitrogen gas, what is the theoretical yield, in grams, of $\mathrm{Na}_{3} \mathrm{~N}$ ?
b. If the reaction in part a has a percent yield of $75.0 \%$, what is the actual yield, in grams, of $\mathrm{Na}_{3} \mathrm{~N}$ ?

Kratika Bhadauria
Kratika Bhadauria
Numerade Educator
01:23

Problem 69

The equation for the reaction of nitrogen and oxygen to form nitrogen oxide is written as $(9.2,9.6)$
$$
\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}(g) \quad \Delta H=+90.2 \mathrm{~kJ}
$$
a. How many kilojoules are required to form $3.00 \mathrm{~g}$ of NO?
b. How many grams of NO form when $66.0 \mathrm{~kJ}$ are absorbed?

Aadit Sharma
Aadit Sharma
Numerade Educator
01:37

Problem 70

The equation for the reaction of iron and oxygen gas to form rust $\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right)$ is written as $(9.2,9.6)$
$$
4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s) \quad \Delta H=-1.7 \times 10^{3} \mathrm{~kJ}
$$
a. How many kilojoules are released when $2.00 \mathrm{~g}$ of Fe reacts?
b. How many grams of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ form when $150 \mathrm{~kJ}$ are released?

Jacquelin Ho
Jacquelin Ho
Numerade Educator
00:39

Problem 71

Each of the following is a reaction that occurs in the cells of the body. Identify each as exothermic or endothermic. (9.6)
a. Succinyl CoA $+\mathrm{H}_{2} \mathrm{O} \longrightarrow$ succinate $+\mathrm{CoA}+37 \mathrm{~kJ}$
b. $\mathrm{GDP}+\mathrm{P}_{\mathrm{i}}+34 \mathrm{~kJ} \longrightarrow \mathrm{GTP}+\mathrm{H}_{2} \mathrm{O}$

Emily Himsel
Emily Himsel
Numerade Educator
00:38

Problem 72

Each of the following is a reaction that occurs in the cells of the body. Identify each as exothermic or endothermic. (9.6)
a. Phosphocreatine $+\mathrm{H}_{2} \mathrm{O} \longrightarrow$ creatine $+\mathrm{P}_{\mathrm{i}}+42.7 \mathrm{~kJ}$
b. Fructose-6-phosphate $+\mathrm{P}_{\mathrm{i}}+16 \mathrm{~kJ} \longrightarrow$

Emily Himsel
Emily Himsel
Numerade Educator
01:34

Problem 73

Use the balanced chemical equation to complete the table: $(9.1,9.2,9.3)$
$$
2 \mathrm{FeS}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{FeO}(s)+2 \mathrm{SO}_{2}(g)
$$

Raghvendra Singh
Raghvendra Singh
Numerade Educator
05:16

Problem 74

Use the balanced chemical equation to complete the table:
$$
\begin{aligned}
&(9.1,9.2,9.3) \\
&\quad 2 \mathrm{C}_{2} \mathrm{H}_{6}(g)+7 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)
\end{aligned}
$$

Nicole Mabante
Nicole Mabante
Numerade Educator
05:37

Problem 75

Chromium and oxygen combine to form chromium(III) oxide. $(9.2,9.3,9.4,9.5)$
$$
4 \mathrm{Cr}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Cr}_{2} \mathrm{O}_{3}(s)
$$
a. How many moles of $\mathrm{O}_{2}$ react with $4.50 \mathrm{~mol}$ of $\mathrm{Cr}$ ?
b. How many grams of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ are produced when $24.8 \mathrm{~g}$ of Cr reacts?
c. When $26.0 \mathrm{~g}$ of $\mathrm{Cr}$ reacts with $8.00 \mathrm{~g} \mathrm{of} \mathrm{} \mathrm{O}_{2}$, how many grams of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ can form?
d. If $74.0 \mathrm{~g}$ of $\mathrm{Cr}$ and $62.0 \mathrm{~g} \mathrm{of} \mathrm{} \mathrm{O}_{2}$ are mixed, and $87.3 \mathrm{~g}$ of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ is actually obtained, what is the percent yield of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ for the reaction?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
05:37

Problem 76

Aluminum and chlorine combine to form aluminum chloride. $(9.2,9.3,9.4,9.5)$
$$
2 \mathrm{Al}(s)+3 \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{AlCl}_{3}(s)
$$
a. How many moles of $\mathrm{Cl}_{2}$ are needed to react with $4.50 \mathrm{~mol}$ of $\mathrm{Al}$ ?
b. How many grams of $\mathrm{AlCl}_{3}$ are produced when $50.2 \mathrm{~g}$ of $\mathrm{Al}$ reacts?
c. When $13.5 \mathrm{~g}$ of $\mathrm{Al}$ reacts with $8.00 \mathrm{~g}$ of $\mathrm{Cl}_{2}$, how many grams of $\mathrm{AlCl}_{3}$ can form?
d. If $45.0 \mathrm{~g}$ of $\mathrm{Al}$ and $62.0 \mathrm{~g}$ of $\mathrm{Cl}_{2}$ are mixed, and $66.5 \mathrm{~g}$ of $\mathrm{AlCl}_{3}$ is actually obtained, what is the percent yield of $\mathrm{AlCl}_{3}$ for the reaction?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:29

Problem 77

The combustion of propyne $\left(\mathrm{C}_{3} \mathrm{H}_{4}\right)$ releases heat when it burns according to the following equation: $(9.2,9.3,9.5)$
$$
\mathrm{C}_{3} \mathrm{H}_{4}(g)+4 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{O}_{2}$ are needed to react completely with $0.225 \mathrm{~mol}$ of $\mathrm{C}_{3} \mathrm{H}_{4}$ ?
b. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are produced from the complete reaction of $64.0 \mathrm{~g}$ of $\mathrm{O}_{2}$ ?
c. How many grams of $\mathrm{CO}_{2}$ are produced from the complete reaction of $78.0 \mathrm{~g}$ of $\mathrm{C}_{3} \mathrm{H}_{4}$ ?
d. If the reaction in part $\mathbf{c}$ produces $186 \mathrm{~g}$ of $\mathrm{CO}_{2}$, what is the percent yield of $\mathrm{CO}_{2}$ for the reaction?

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
14:10

Problem 78

Butane gas $\left(\mathrm{C}_{4} \mathrm{H}_{10}\right)$ burns according to the following equation: $(9.2,9.3,9.5)$
$$
2 \mathrm{C}_{4} \mathrm{H}_{10}(g)+13 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 8 \mathrm{CO}_{2}(g)+10 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{H}_{2} \mathrm{O}$ are produced from the complete reaction of $2.50 \mathrm{~mol}$ of $\mathrm{C}_{4} \mathrm{H}_{10}$ ?
b. How many grams of $\mathrm{O}_{2}$ are needed to react completely with $22.5 \mathrm{~g}$ of $\mathrm{C}_{4} \mathrm{H}_{10}$ ?
c. How many grams of $\mathrm{CO}_{2}$ are produced from the complete reaction of $55.0 \mathrm{~g}$ of $\mathrm{C}_{4} \mathrm{H}_{10}$ ?
d. If the reaction in part c produces $145 \mathrm{~g}$ of $\mathrm{CO}_{2}$, what is the percent yield of $\mathrm{CO}_{2}$ for the reaction?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:48

Problem 79

Sulfur trioxide decomposes to sulfur and oxygen. $(9.2,9.6)$
$$
2 \mathrm{SO}_{3}(g) \longrightarrow 2 \mathrm{~S}(s)+3 \mathrm{O}_{2}(g) \quad \Delta H=+790 \mathrm{~kJ}
$$
a. Is the reaction exothermic or endothermic?
b. How many kilojoules are required when $1.5 \mathrm{~mol}_{\text {of } \mathrm{SO}_{3}}$ reacts?
c. How many kilojoules are required when $150 \mathrm{~g}$ of $\mathrm{O}_{2}$ is formed?

Nicole Smina
Nicole Smina
Numerade Educator
01:51

Problem 80

When hydrogen peroxide $\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)$ is used in rocket fuels, it produces water, oxygen, and heat. $(9.2,9.6)$
$$
2 \mathrm{H}_{2} \mathrm{O}_{2}(l) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g) \quad \Delta H=-196 \mathrm{~kJ}
$$
a. Is the reaction exothermic or endothermic?
b. How many kilojoules are released when $2.50 \mathrm{~mol}$ of $\mathrm{H}_{2} \mathrm{O}_{2}$ reacts?
c. How many kilojoules are released when $275 \mathrm{~g}$ of $\mathrm{O}_{2}$ is produced?

Nicole Smina
Nicole Smina
Numerade Educator
01:33

Problem 81

Calculate the energy change for the reaction
$$
\begin{array}{ll}
\mathrm{NH}_{4} \mathrm{Cl}(s) \longrightarrow \mathrm{NH}_{3}(g)+\mathrm{HCl}(g) \text { from the following: (9.6) } \\
\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{HCl}(g) & \Delta H=-184 \mathrm{~kJ} \\
\mathrm{~N}_{2}(g)+4 \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NH}_{4} \mathrm{Cl}(s) & \Delta H=-631 \mathrm{~kJ} \\
\mathrm{~N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g) & \Delta H=-296 \mathrm{~kJ}
\end{array}
$$

David Collins
David Collins
Numerade Educator
View

Problem 82

Calculate the energy change for the reaction
$\mathrm{Mg}(s)+\mathrm{N}_{2}(g)+3 \mathrm{O}_{2}(g) \longrightarrow \mathrm{Mg}^{2}\left(\mathrm{NO}_{3}\right)_{2}(s)$ from the following: (9.6)
$$
\begin{array}{ll}
8 \mathrm{Mg}(s)+\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(s) \longrightarrow \mathrm{Mg}_{3} \mathrm{~N}_{2}(s)+6 \mathrm{MgO}(s) \\
& \Delta H=-3281 \mathrm{~kJ} \\
\mathrm{Mg}_{3} \mathrm{~N}_{2}(s) \longrightarrow 3 \mathrm{Mg}(s)+\mathrm{N}_{2}(g) & \Delta H=+461 \mathrm{~kJ} \\
2 \mathrm{MgO}(s) \longrightarrow 2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) & \Delta H=+1204 \mathrm{~kJ}
\end{array}
$$

Ronald Prasad
Ronald Prasad
Numerade Educator
04:15

Problem 83

In the body, the amino acid glycine $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}\right)$ reacts according to the following equation: (9.3)
$2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow$
Glycine $\quad 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CH}_{4} \mathrm{~N}_{2} \mathrm{O}(a q)$
UreaIn the body, the amino acid glycine $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}\right)$ reacts according to the following equation: (9.3)
$2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow$
Glycine $\quad 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CH}_{4} \mathrm{~N}_{2} \mathrm{O}(a q)$
Urea
a. How many grams of $\mathrm{O}_{2}$ are needed to react with $15.0 \mathrm{~g}$ of glycine?
b. How many grams of urea are produced from $15.0 \mathrm{~g}$ of glycine?
c. How many grams of $\mathrm{CO}_{2}$ are produced from $15.0 \mathrm{~g}$ of glycine?

Sima Sarker
Sima Sarker
Numerade Educator
05:11

Problem 84

In the body, ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\right)$ reacts according to the following equation: (9.3)
$$
\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)
$$
Ethanol
a. How many grams of $\mathrm{O}_{2}$ are needed to react with $8.40 \mathrm{~g}$ of ethanol?
b. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are produced from $8.40 \mathrm{~g}$ of ethanol?
c. How many grams of $\mathrm{CO}_{2}$ are produced from $8.40 \mathrm{~g}$ of ethanol?

Ashley Brady
Ashley Brady
Numerade Educator
02:48

Problem 85

In photosynthesis, glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ and $\mathrm{O}_{2}$ are produced from $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O}$. Glucose from starches is the major fuel for the body. $(9.3,9.6)$
$6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)+680 \mathrm{kcal} \longrightarrow \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(a q)+6 \mathrm{O}_{2}(g)$
Glucose
a. Is the reaction exothermic or endothermic?
b. How many grams of glucose are produced from $18.0 \mathrm{~g}$ of $\mathrm{CO}_{2}$ ?
c. How much heat, in kilojoules, is needed to produce $25.0 \mathrm{~g}$ of $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ ?

Nicole Smina
Nicole Smina
Numerade Educator
05:22

Problem 86

Ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\right)$ reacts in the body using the following equation: $(9.3,9.5)$
$\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+327 \mathrm{kcal}$ Ethanol
a. Is the reaction exothermic or endothermic?
b. How much heat, in kilocalories, is produced when $5.00 \mathrm{~g}$ of ethanol reacts with $\mathrm{O}_{2}$ gas?
c. How many grams of ethanol react if $1250 \mathrm{~kJ}$ are produced?

Dennis Howard
Dennis Howard
Numerade Educator