Introduction to General, Organic and Biochemistry

Frederick A. Bettelheim, William H. Brown, Mary K. Campbell

Chapter 5

Gases, Liquids, and Solids - all with Video Answers

Educators

Chapter Questions

Problem 1

A gas occupies $3.8 \mathrm{L}$ at 0.70 atm pressure. If we expand the volume at constant temperature to $6.5 \mathrm{L}$, what is the final pressure?

David Collins

David Collins

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Problem 2

A constant volume of oxygen gas, $\mathrm{O}_{2},$ is heated from $120 .^{\circ} \mathrm{C}$ to $212^{\circ} \mathrm{C}$. The final pressure is 20.3 atm. What was the initial pressure?

David Collins

Numerade Educator

Problem 3

A gas is expanded from an initial volume of $20.5 \mathrm{L}$ at 0.92 atm at room temperature $\left(23.0^{\circ} \mathrm{C}\right)$ to a final volume of 340.6 L. During the expansion, the gas cools to $12.0^{\circ} \mathrm{C}$. What is the new pressure?

David Collins

Numerade Educator

Problem 4

If $2.00 \mathrm{mol}$ of $\mathrm{NO}$ gas occupies $10.0 \mathrm{L}$ at $295 \mathrm{K}$, what is the pressure of the gas in atmospheres?

David Collins

Numerade Educator

Problem 5

A certain quantity of neon gas is under 1.05 atm pressure at $303 \mathrm{K}$ in a $10.0 \mathrm{L}$ vessel. How many moles of neon are present?

David Collins

Numerade Educator

Problem 6

An unknown amount of He gas occupies 30.5 L at 2.00 atm pressure and $300 .$ K. What is the weight of the gas in the container?

Shivani Beall

Numerade Educator

Problem 7

A vessel under 2.015 atm pressure contains nitrogen, $\mathrm{N}_{2}$, and water vapor, $\mathrm{H}_{2} \mathrm{O}$. The partial pressure of $\mathrm{N}_{2}$ is 1.908 atm. What is the partial pressure of the water vapor?

David Collins

Numerade Educator

Problem 8

Will the molecules in each set form a hydrogen bond between them?
(a) A molecule of water and a molecule of methanol, $\mathrm{CH}_{3} \mathrm{OH}$
(b) Two molecules of methane, CH

David Collins

Numerade Educator

Problem 9

What mass of water at $100^{\circ} \mathrm{C}$ can be vaporized by the addition of 45.0 kcal of heat?

David Collins

Numerade Educator

Problem 10

The specific heat of iron is 0.11 callg $\cdot^{\circ} \mathrm{C}$ (Table $1-4$ ). The heat of fusion of iron-that is, the heat required to convert iron from a solid to a liquid at its melting point- -is 63.7 callg. Iron melts at $1530^{\circ} \mathrm{C}$. How much heat must be added to $1.0 \mathrm{g}$ of iron at $25^{\circ} \mathrm{C}$ to completely melt it?

David Collins

Numerade Educator

Problem 11

What will happen to water vapor if it is cooled from $100^{\circ} \mathrm{C}$ to $-30^{\circ} \mathrm{C}$ while the pressure stays at 1 atm?

David Collins

Numerade Educator

Problem 12

A weather report says that the barometric pressure is 29.5 inches of mercury. What is this pressure in atmospheres?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 13

Use the kinetic molecular theory to explain why, at constant temperature, the pressure of a gas increases as its volume is decreased.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 14

Use the kinetic molecular theory to explain why the pressure of a gas in a fixed-volume container increases as its temperature is increased.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 15

Name three ways by which the volume of a gas can be decreased.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 16

Answer true or false.
(a) For a sample of gas at constant temperature, its pressure multiplied by its volume is a constant.
(b) For a sample of gas at constant temperature, increasing the pressure increases the volume.
(c) For a sample of gas at constant temperature, $P_{1} / V_{1}=P_{2} / V_{2}$
(d) As a gas expands at constant temperature, its volume increases.
(e) The volume of a sample of gas at constant pressure is directly proportional to its temperature-the higher its temperature, the greater its volume.
(f) A hot-air balloon rises because hot air is less dense than cooler air.
(g) For a gas sample in a container of fixed volume, an increase in temperature results in an increase in pressure.
(h) For a gas sample in a container of fixed volume, $P \times T$ is a constant.
(i) When steam at $100^{\circ} \mathrm{C}$ in an autoclave is heated to $120^{\circ} \mathrm{C},$ the pressure within the autoclave increases.
(j) When a gas sample in a flexible container at constant pressure at $25^{\circ} \mathrm{C}$ is heated to $50^{\circ} \mathrm{C}$, its volume doubles.
(k) Lowering the diaphragm causes the chest cavity to increase in volume and the pressure of air in the lungs to decrease.
(l) Raising the diaphragm decreases the volume of the chest cavity and forces air out of the lungs.

Yash Ramgopal

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Problem 17

A sample of gas has a volume of $6.20 \mathrm{L}$ at $20^{\circ} \mathrm{C}$ at a pressure of 1.10 atm. What is its volume at the same temperature and at a pressure of 0.925 atm?

Pronoy Sinha

Numerade Educator

Problem 18

Methane gas is compressed from 20. L to 2.5 L at a constant temperature. The final pressure is 12.2 atm. What was the original pressure?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 19

A gas syringe at $20^{\circ} \mathrm{C}$ contains $20.0 \mathrm{mL}$ of $\mathrm{CO}_{2}$ gas. The pressure of the gas in the syringe is 1.0 atm. What is the pressure in the syringe at $20^{\circ} \mathrm{C}$ if the plunger is depressed to $10.0 \mathrm{mL} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 20

Suppose that the pressure in an automobile tire is 2.30 atm at a temperature of $20.0^{\circ} \mathrm{C}$. What will the pressure in the tire be if after 10 miles of driving the temperature of the tire increases to $47.0^{\circ} \mathrm{C} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 21

A sample of $23.0 \mathrm{L}$ of $\mathrm{NH}_{3}$ gas at $10.0^{\circ} \mathrm{C}$ is heated at constant pressure until it fills a volume of $50.0 \mathrm{L}$ What is the new temperature in $^{\circ} \mathrm{C} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 22

If a sample of 4.17 L of ethane gas, $\mathrm{C}_{2} \mathrm{H}_{6},$ at $725^{\circ} \mathrm{C}$ is cooled to $175^{\circ} \mathrm{C}$ at constant pressure, what is the new volume?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 23

A sample of $\mathrm{SO}_{2}$ gas has a volume of $5.2 \mathrm{L}$. It is heated at constant pressure from $30,$ to $90 .^{\circ} \mathrm{C}$. What is its new volume?

Shalini Tyagi

Numerade Educator

Problem 24

A sample of $\mathrm{B}_{2} \mathrm{H}_{6}$ gas in a 35 -mL container is at a pressure of $450 .$ mm Hg and a temperature of $625^{\circ} \mathrm{C}$ If the gas is allowed to cool at constant volume until the pressure is $375 \mathrm{mm}$ Hg, what is the new temperature in $^{\circ} \mathrm{C} ?$

David Collins

Numerade Educator

Problem 25

A gas in a bulb as in Figure $5-3$ registers a pressure of $833 \mathrm{mm} \mathrm{Hg}$ in the manometer in which the reference arm of the U-shaped tube (A) is sealed and evacuated. What will the difference in the mercury levels be if the reference arm of the U-shaped tube is open to atmospheric pressure $(760 \mathrm{mm} \mathrm{Hg}) ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 26

In an autoclave, a constant amount of steam is generated at a constant volume. Under 1.00 atm pressure, the steam temperature is $100 .^{\circ} \mathrm{C}$. What pressure setting should be used to obtain a $165^{\circ} \mathrm{C}$ steam temperature for the sterilization of surgical instruments?

David Collins

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Problem 27

A sample of the inhalation anesthetic gas Halothane, $\mathrm{C}_{2} \mathrm{HBrCIF}_{3},$ in a $500-\mathrm{mL}$ cylinder has a pressure of 2.3 atm at $0^{\circ} \mathrm{C}$. What will be the pressure of the gas if its temperature is warmed to $37^{\circ} \mathrm{C}$ (body temperature)?

David Collins

Numerade Educator

Problem 28

Complete this table:
$$\begin{array}{|l|l|l|l|l|l|}\hline V_{1} & T_{1} & {}{} {P_{1}} & {}{} {V_{2}} & {}{} {T_{2}} & {}{} {P_{2}} \\
\hline 546 \mathrm{L} & 43^{\circ} \mathrm{C} & 6.5 \mathrm{atm} & & 65^{\circ} \mathrm{C} & 1.9 \mathrm{atm} \\
\hline 43 \mathrm{mL} & -56^{\circ} \mathrm{C} & 865 \text { torr } & & 43^{\circ} \mathrm{C} & 1.5 \mathrm{atm} \\
\hline 4.2 \mathrm{L} & 234 \mathrm{K} & 0.87 \mathrm{atm} & 3.2 \mathrm{L} & 29^{\circ} \mathrm{C} & \\
\hline 1.3 \mathrm{L} & 25^{\circ} \mathrm{C} & 740 \mathrm{mm} \mathrm{Hg} & & 0^{\circ} \mathrm{C} & 1.0 \mathrm{atm} \\
\hline\end{array}$$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 29

Complete this table:
$$\begin{array}{|l|c|c|c|c|c|}\hline V_{1} & T_{1} & P_{1} & V_{2} & T_{2} & P_{2} \\
\hline 6.35 \mathrm{L} & 10^{\circ} \mathrm{C} & 0.75 \mathrm{atm} & & 0^{\circ} \mathrm{C} & 1.0 \mathrm{atm} \\
\hline 75.6 \mathrm{L} & 0^{\circ} \mathrm{C} & 1.0 \mathrm{atm} & & 35^{\circ} \mathrm{C} & 735 \mathrm{torr} \\
\hline 1.06 \mathrm{L} & 75^{\circ} \mathrm{C} & 0.55 \mathrm{atm} & 3.2 \mathrm{L} & 0^{\circ} \mathrm{C} & \\
\hline\end{array}$$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 30

A balloon filled with $1.2 \mathrm{L}$ of helium at $25^{\circ} \mathrm{C}$ and 0.98 atm pressure is submerged in liquid nitrogen at $-196^{\circ} \mathrm{C}$. Calculate the final volume of the helium in the balloon.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 31

A balloon used for atmospheric research has a volume of $1 \times 10^{6}$ L. Assume that the balloon is filled with helium gas at STP and then allowed to ascend to an altitude of $10 \mathrm{km}$, where the pressure of the atmosphere is $243 \mathrm{mm}$ Hg and the temperature is $-33^{\circ} \mathrm{C} .$ What will the volume of the balloon be under these atmospheric conditions?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 32

A gas occupies $56.44 \mathrm{L}$ at 2.00 atm and $310 .$ K. If the gas is compressed to $23.52 \mathrm{L}$ and the temperature is lowered to $281 \mathrm{K}$, what is the new pressure?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 33

A certain quantity of helium gas is at a temperature of $27^{\circ} \mathrm{C}$ and a pressure of 1.00 atm. What will the new temperature be if its volume is doubled at the same time that its pressure is decreased to one-half its original value?

Gene Schneider

Numerade Educator

Problem 34

A sample of $30.0 \mathrm{mL}$ of krypton gas, $\mathrm{Kr}$, is at $756 \mathrm{mm} \mathrm{Hg}$ and $25.0^{\circ} \mathrm{C} .$ What is the new volume if the pressure is decreased to $325 \mathrm{mm}$ Hg and the temperature is decreased to $-12.5^{\circ} \mathrm{C} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 35

A 26.4 -mL sample of ethylene gas, $\mathrm{C}_{2} \mathrm{H}_{4},$ has a pressure of 2.50 atm at $2.5^{\circ} \mathrm{C}$. If the volume is increased to $36.2 \mathrm{mL}$ and the temperature is raised to $10^{\circ} \mathrm{C}$ what is the new pressure?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 36

Answer true or false.
(a) Avogadro's law states that equal volumes of gas at the same temperature and pressure contain equal numbers of molecules.
(b) At STP, one mole of uranium hexafluoride (UF $_{6}$, MW 352 amu), the gas used in uranium enrichment programs, occupies a volume of $352 \mathrm{L}$
(c) If two gas samples have the same temperature, volume, and pressure, then both contain the same number of molecules.
(d) The value of Avogadro's number is $6.02 \times 10^{23} \mathrm{g} / \mathrm{mol}$
(e) Avogadro's number is valid only for gases at STP.
(f) The ideal gas law is $P V=n R T$.
(g) When using the ideal gas law for calculations, temperature must be in degrees Celsius.
(h) If one mole of ethane $\left(\mathrm{CH}_{3} \mathrm{CH}_{3}\right)$ gas occupies $20.0 \mathrm{L}$ at 1.00 atm, the temperature of the gas is $244 \mathrm{K}$
(i) One mole of helium (MW 4.0 amu) gas at STP occupies twice the volume of one mole of hydrogen $(\mathrm{MW} 2.0 \mathrm{amu})$

David Collins

Numerade Educator

Problem 37

A sample of a gas at $77^{\circ} \mathrm{C}$ and 1.33 atm occupies a volume of $50.3 \mathrm{L}$
(a) How many moles of the gas are present?
(b) Does your answer depend on knowing what gas it is?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 38

What is the volume in liters occupied by $1.21 \mathrm{g}$ of Freon-12 gas, $\mathrm{CCl}_{2} \mathrm{F}_{2},$ at 0.980 atm and $35^{\circ} \mathrm{C} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 39

An 8.00 -g sample of a gas occupies $22.4 \mathrm{L}$ at 2.00 atm and $273 \mathrm{K}$. What is the molar mass of the gas?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 40

What volume is occupied by $5.8 \mathrm{g}$ of propane gas, $\mathrm{C}_{3} \mathrm{H}_{6},$ at $23^{\circ} \mathrm{C}$ and 1.15 atm pressure?

David Collins

Numerade Educator

Problem 41

Does the density of a gas increase, decrease, or stay the same as the pressure increases at constant temperature? As the temperature increases at constant pressure?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 42

What volume in milliliters does 0.275 g of uranium hexafluoride gas, UF $_{6}$, occupy at its boiling point of $56^{\circ} \mathrm{C}$ at 365 torr?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 43

A hyperbaric chamber has a volume of $200 .$ L.
(a) How many moles of oxygen are needed to fill the chamber at room temperature $\left(23^{\circ} \mathrm{C}\right)$ and 3.00 atm pressure?
(b) How many grams of oxygen are needed?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 44

One breath of air has a volume of $2 \mathrm{L}$ at STP. If air contains $20.9 \%$ oxygen, how many molecules of oxygen are in one breath?

Madeline Currie

Madeline Currie

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Problem 45

An average pair of lungs has a volume of 5.5 L. If the air they contain is $21 \%$ oxygen, how many molecules of $\mathrm{O}_{2}$ do the lungs contain at $1.1 \mathrm{atm}$ and $37^{\circ} \mathrm{C} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 46

Calculate the molar mass of a gas if $3.30 \mathrm{g}$ of the gas occupies $660 . \mathrm{mL}$ at $735 \mathrm{mm} \mathrm{Hg}$ and $27^{\circ} \mathrm{C}$.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 47

The three main components of dry air and the percentage of each are $\mathrm{N}_{2}(78.08 \%), \mathrm{O}_{2}(20.95 \%),$ and $\mathrm{Ar}(0.93 \%)$
(a) Calculate the mass of one mole of air.
(b) Given the mass of one mole of air, calculate the density of air in $\mathrm{g} / \mathrm{L}$ at $\mathrm{STP}$
.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 48

The density of Freon-12, $\mathrm{CCl}_{2} \mathrm{F}_{2}$ at STP is $4.99 \mathrm{g} / \mathrm{L}$, which means that it is approximately four times more dense than air. Show how the kinetic molecular theory of gases accounts for the fact that although Freon-12 is more dense than air, it nevertheless finds its way to the stratosphere, where it is implicated in the destruction of Earth's protective ozone layer:

David Collins

Numerade Educator

Problem 49

Calculate the density in g/L of each of these gases at STP. Which gases are denser than air as calculated in Problem $5-47(\mathrm{b}) ?$ Which are less dense than air?
$(a) S O_{2}$
(b) $\mathrm{CH}_{4}$
(c) $\mathrm{H}_{2}$
(d) $\mathrm{He}$
(e) $\mathrm{CO}_{2}$

David Collins

Numerade Educator

Problem 50

How many molecules of CO are in $100 .$ L of $\mathrm{CO}$ at $\mathrm{STP} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 51

The density of liquid octane, $\mathrm{C}_{8} \mathrm{H}_{18},$ is $0.7025 \mathrm{g} / \mathrm{mL}$ If $1.00 \mathrm{mL}$ of liquid octane is vaporized at $100^{\circ} \mathrm{C}$ and 725 torr, what volume does the vapor occupy?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 52

The density of acetylene gas, $\mathrm{C}_{2} \mathrm{H}_{2},$ in a $4-\mathrm{L}$ container at $0^{\circ} \mathrm{C}$ and 2 atm pressure is $0.02 \mathrm{g} / \mathrm{mL}$. What would be the density of the gas under identical temperature and pressure if the container were partitioned into two 2 -L compartments?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 53

Sodium metal reacts explosively with hydrochloric acid, $\mathrm{HCl}(a q),$ as shown in the following chemical equation:
\[2 \mathrm{Na}(s)+2 \mathrm{HCl}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{H}_{2}(g)\]
What volume of $\mathrm{H}_{2}(g)$ is produced when 3.50 g of $\mathrm{Na}(s)$ is reacted with an excess of hydrochloric acid at a temperature of $18^{\circ} \mathrm{C}$ and a pressure of 0.995 atm?

David Collins

Numerade Educator

Problem 54

Automobile air bags are inflated by nitrogen gas. When a significant collision occurs, an electronic sensor triggers the decomposition of sodium azide to form nitrogen gas and sodium metal. The nitrogen gas then inflates nylon bags, which protect the driver and front-seat passenger from impact with the dashboard and windshield.
\[2 \mathrm{NaN}_{3}(s) \longrightarrow 2 \mathrm{Na}(s)+3 \mathrm{N}_{2}(g)\]
Sodium azide
What volume of nitrogen gas measured at 1 atm and $27^{\circ} \mathrm{C}$ is formed by the decomposition of $100 .$ g of sodium azide?

David Collins

Numerade Educator

Problem 55

Answer true or false.
(a) Partial pressure is the pressure that a gas in a container would exert if it were alone in the container.
(b) The units of partial pressure are grams per liter.
(c) Dalton's law of partial pressures states that the total pressure of a mixture of gases is the sum of the partial pressures of each gas.
(d) If 1 mole of $\mathrm{CH}_{4}$ gas at $\mathrm{STP}$ is added to $22.4 \mathrm{L}$ of $\mathrm{N}_{2}$ at $\mathrm{STP}$, the final pressure in the $22.4 \mathrm{L}$ container will be 1.00 atm.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 56

The three main components of dry air and the percentage of each are nitrogen $(78.08 \%),$ oxygen $(20.95 \%),$ and argon $(0.93 \%)$
(a) Calculate the partial pressure of each gas in a sample of dry air at $760 \mathrm{mm} \mathrm{Hg}$
(b) Calculate the total pressure exerted by these three gases combined.

David Collins

Numerade Educator

Problem 57

Air in the trachea contains oxygen $(19.4 \%),$ carbon dioxide $(0.4 \%),$ water vapor $(6.2 \%),$ and nitrogen $(74.0 \%) .$ If the pressure in the trachea is assumed to be 1.0 atm, what are the partial pressures of these gases in this part of the body?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 58

The partial pressures of a mixture of gases are as follows: oxygen, $210 \mathrm{mm}$ Hg; nitrogen, $560 \mathrm{mm} \mathrm{Hg}$ and carbon dioxide, $15 \mathrm{mm}$ Hg. The total pressure of the gas mixture was $790 \mathrm{mm}$ Hg. Is there another gas present in the mixture?

David Collins

Numerade Educator

Problem 59

Answer true or false.
(a) According to the kinetic molecular theory, gas particles have mass but no volume.
(b) According to the kinetic molecular theory, the average kinetic energy of gas particles is proportional to the temperature in degrees Celsius.
(c) According to the kinetic molecular theory, when gas particles collide, they bounce off each other with no change in total kinetic energy.
(d) According to the kinetic molecular theory, there are only weak intramolecular forces of attraction between gas particles.
(e) According to the kinetic molecular theory, the pressure of a gas in a container is the result of collisions of gas particles on the walls of the container.
(f) Warming a gas results in an increase in the average kinetic energy of its particles.
(g) When a gas is compressed, the increase in its pressure is the result of an increase in the number of collisions of its particles on the walls of the container.
(h) The kinetic molecular theory describes the behavior of ideal gases, of which there are only a few.
(i) As the temperature and volume of a gas increase, the behavior of the gas becomes more like the behavior predicted by the ideal gas law.
(j) If the assumptions of the kinetic molecular theory of gases are correct, then there is no combination of temperature and pressure at which a gas would become liquid.

Yash Ramgopal

Numerade Educator

Problem 60

Compare and contrast Dalton's atomic theory and the kinetic molecular theory.

Yash Ramgopal

Numerade Educator

Problem 61

Answer true or false.
(a) Of the forces of attraction between particles, London dispersion forces are the weakest and covalent bonds are the strongest.
(b) All covalent bonds have approximately the same
energy.
(c) London dispersion forces arise because of the attraction of temporary induced dipoles.
(d) In general, London dispersion forces increase as molecular size increases.
(e) London dispersion forces occur only between polar molecules - they do not occur between nonpolar atoms or molecules.
(f) The existence of London dispersion forces accounts for the fact that even small, nonpolar particles such as $\mathrm{Ne}, \mathrm{He},$ and $\mathrm{H}_{2}$ can be liquefied if the temperature is low enough and the pressure is high enough.
(g) For nonpolar gases at STP, the average kinetic energy of its particles is greater than the force of attraction between gas particles.
(h) Dipole-dipole interaction is the attraction between the positive end of one dipole and the negative end of another.
(i) Dipole-dipole interactions exist between CO molecules but not between $\mathrm{CO}_{2}$ molecules.
(j) If two polar molecules have approximately the same molecular weight, the strength of the dipole-dipole interactions between the molecules of each will be approximately the same.
(k) Hydrogen bonding refers to the single covalent bond between the two hydrogen atoms in $\mathrm{H}-\mathrm{H}$
(l) The strength of hydrogen bonding in liquid water is approximately the same as that of an $\mathrm{O}-\mathrm{H}$ covalent bond in water.
(m) Hydrogen bonding, dipole-dipole interactions, and London dispersion forces have in common that the forces of attraction between particles are all electrostatic (positive to negative and negative to positive)
(n) Water $\left(\mathrm{H}_{2} \mathrm{O}, \mathrm{bp} 100^{\circ} \mathrm{C}\right)$ has a higher boiling point than hydrogen sulfide $\left(\mathrm{H}_{2} \mathrm{S}, \mathrm{bp}-61^{\circ} \mathrm{C}\right)$ because the hydrogen bonding between $\mathrm{H}_{2} \mathrm{O}$ molecules is stronger than that between $\mathrm{H}_{2} \mathrm{S}$ molecules.
(o) The hydrogen bonding among molecules containing $\mathrm{N}-\mathrm{H}$ groups is stronger than that among molecules containing $\mathrm{O}-\mathrm{H}$ groups.

David Collins

Numerade Educator

Problem 62

Which forces are stronger, intramolecular covalent bonds or intermolecular hydrogen bonds?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 63

Under which condition does water vapor behave most ideally?
(a) 0.5 atm, $400 \mathrm{K}$
(b) 4 atm, $500 \mathrm{K}$
(c) $0.01 \mathrm{atm}, 500 \mathrm{K}$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 64

Can water and dimethyl sulfoxide, $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{S}=\mathrm{O}$ molecules form hydrogen bonds between them?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 65

What kind of intermolecular interactions take place in (a) liquid $\mathrm{CCl}_{4}$ and (b) liquid CO? Which will have the highest surface tension?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 66

Ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$, and carbon dioxide, $\mathrm{CO}_{2}$, have approximately the same molecular weight, yet carbon dioxide is a gas at STP and ethanol is a liquid. How do you account for this difference in physical property?

David Collins

Numerade Educator

Problem 67

Can dipole-dipole interactions ever be weaker than London dispersion forces? Explain.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 68

Which compound has a higher boiling point: butane, $\mathrm{C}_{4} \mathrm{H}_{10},$ or hexane, $\mathrm{C}_{6} \mathrm{H}_{14} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 69

Answer true or false.
(a) The ideal gas law assumes that there are no attractive forces between molecules. If this were true, then there would be no liquids.
(b) Unlike a gas, whose molecules move freely in any direction, molecules in a liquid are locked into fixed positions, giving the liquid a constant shape.
(c) Surface tension is the force that prevents a liquid from being stretched.
(d) Surface tension creates an elastic-like layer on the surface of a liquid.
(e) Water has a high surface tension because $\mathrm{H}_{2} \mathrm{O}$ is a small molecule.
(f) Vapor pressure is proportional to temperature as the temperature of a liquid sample increases, its vapor pressure also increases.
(g) When molecules evaporate from a liquid, the temperature of the liquid drops.
(h) Evaporation is a cooling process because it leaves fewer molecules with high kinetic energy in the liquid state.
(i) The boiling point of a liquid is the temperature at which its vapor pressure equals the atmospheric pressure.
(j) As the atmospheric pressure increases, the boiling point of a liquid increases.
(k) The temperature of boiling water is related to how vigorously it is boiling-the more vigorous the boiling, the higher the temperature of the water.
(1) The most important factor determining the relative boiling points of liquids is molecular weight-the greater the molecular weight, the higher the boiling point.
$(\mathrm{m})$ Ethanol $\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}, \mathrm{bp} 78.5^{\circ} \mathrm{C}\right)$ has a greater
vapor pressure at $25^{\circ} \mathrm{C}$ than water $\left(\mathrm{H}_{2} \mathrm{O}\right.$ bp $\left.100^{\circ} \mathrm{C}\right)$
(n) Hexane $\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}, \mathrm{bp} 69^{\circ} \mathrm{C}\right)$
has a higher boiling point than methane $\left(\mathrm{CH}_{4}\right.$ $\left.\mathrm{bp}-164^{\circ} \mathrm{C}\right)$ because hexane has more sites for hydrogen bonding between its molecules than does methane.
(o) A water molecule can participate in hydrogen bonding through each of its hydrogen atoms and through its oxygen atom.
(p) For nonpolar molecules of comparable molecular weight, the more compact the shape of the molecule, the higher its boiling point.

David Collins

Numerade Educator

Problem 70

The melting point of chloroethane, $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Cl}$, is $-136^{\circ} \mathrm{C}$ and its boiling point is $12^{\circ} \mathrm{C}$. Is chloroethane a gas, a liquid, or a solid at STP?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 71

Answer true or false.
(a) Formation of a liquid from a solid is called melting; formation of a solid from a liquid is called crystallization.
(b) Most solids have a higher density than their liquid forms.
(c) Molecules in a solid are locked into fixed positions.
(d) Each element has one and only one solid (crystalline) form.
(e) Diamond and graphite are both crystalline forms of carbon.
(f) Diamond consists of hexagonal crystals of carbon arranged in a repeating pattern.
(g) The nano in nanotube refers to the structure dimensions, which are in the nanometer $\left(10^{-9} \mathrm{m}\right)$ range.
(h) Nanotubes have lengths up to $1 \mathrm{nm}$.
(i) A buckyball (C $_{80}$ ) has a diameter of $1 \mathrm{nm}$.
(j) All solids, if heated to a high enough temperature, can be melted.
(k) Glass is an amorphous solid.

David Collins

Numerade Educator

Problem 72

Identify the type of crystalline solid (i.e., ionic, molecular, metallic, network covalent, polymeric) formed by each of the following:
(a) glucose, $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$
(b) silver, Ag
(c) silicon carbide, SiC
(d) bottle containing Arrowhead" brand mountain spring water
(e) potassium iodide, KI
(f) elemental sulfur powder, $\mathrm{S}_{8}$

David Collins

Numerade Educator

Problem 73

Answer true or false.
(a) A phase change from solid to liquid is called melting.
(b) A phase change from liquid to gas is called boiling.
(c) If heat is added slowly to a mixture of ice and liquid water, the temperature of the sample gradually increases until all of the ice is melted.
(d) Heat of fusion is the heat required to melt 1 g of a solid.
(e) Heat of vaporization is the heat required to evaporate $1 \mathrm{g}$ of liquid at the normal boiling point of the liquid.
(f) Steam burns are more damaging to the skin than hot-water burns because the specific heat of steam is so much higher than the specific heat of hot water.
(g) The heat of vaporization of water is approximately the same as its heat of fusion.
(h) The specific heat of water is the heat required to raise the temperature of 1 g of water from $0^{\circ} \mathrm{C}$ to $100^{\circ} \mathrm{C}$
(i) Melting a solid is an exothermic process; crystallization of a liquid is an endothermic process.
(j) Melting a solid is a reversible process; the solid can be converted to a liquid and the liquid back to a solid with no change in composition of the sample.
(k) Sublimation is a phase change from solid directly to gas.

David Collins

Numerade Educator

Problem 74

Calculate the specific heat (Section $1-9$ ) of gaseous Freon-12, $\mathrm{CCl}_{2} \mathrm{F}_{2},$ if it requires $170 .$ cal to change the temperature of $36.6 \mathrm{g}$ of Freon- 12 from $30 .^{\circ} \mathrm{C}$ to $50 .^{\circ} \mathrm{C}$.

David Collins

Numerade Educator

Problem 75

The heat of vaporization of liquid Freon-12, $\mathrm{CCl}_{2} \mathrm{F}_{2}$ is $4.71 \mathrm{kcal} / \mathrm{mol}$. Calculate the energy required to vaporize $39.2 \mathrm{g}$ of this compound. The molecular weight of Freon-12 is 120.9 amu.

David Collins

Numerade Educator

Problem 76

The specific heat (Section $1-9$ ) of mercury is $0.0332 \mathrm{cal} / \mathrm{g} \cdot^{\circ} \mathrm{C} .$ Calculate the energy necessary to raise the temperature of one mole of liquid mercury by $36^{\circ} \mathrm{C}$.

David Collins

Numerade Educator

Problem 77

Using Figure $5-14$, estimate the vapor pressure of ethanol at
(a) $30^{\circ} \mathrm{C},$
(b) $40^{\circ} \mathrm{C},$ and
(c) $60^{\circ} \mathrm{C}$

David Collins

Numerade Educator

Problem 78

$\mathrm{CH}_{4}$ and $\mathrm{H}_{2} \mathrm{O}$ have about the same molecular weight. Which has the higher vapor pressure at room temperature? Explain.

David Collins

Numerade Educator

Problem 79

The normal boiling point of a substance depends on both the mass of the molecule and the attractive forces between molecules. Arrange the compounds in each set in order of increasing boiling point and explain your answer:
(a) $\mathrm{HCl}, \mathrm{HBr}, \mathrm{HI}$
(b) $\mathrm{O}_{2}, \mathrm{HCl}, \mathrm{H}_{2} \mathrm{O}_{2}$

David Collins

Numerade Educator

Problem 80

Refer to Figure $5-19 .$ How many calories are required to bring one mole of ice at $0^{\circ} \mathrm{C}$ to a liquid state at room temperature $\left(23^{\circ} \mathrm{C}\right) ?$

David Collins

Numerade Educator

Problem 81

Compare the number of calories absorbed when $100 .$ g of ice at $0^{\circ} \mathrm{C}$ is changed to liquid water at $37^{\circ} \mathrm{C}$ with the number of calories absorbed when $100 .$ g of liquid water is warmed from $0^{\circ} \mathrm{C}$ to $37^{\circ} \mathrm{C}$.

David Collins

Numerade Educator

Problem 82

(a) How much energy is released when $10 .$ g of steam at $100^{\circ} \mathrm{C}$ is condensed and cooled to body temperature $\left(37^{\circ} \mathrm{C}\right) ?$
(b) How much energy is released when $100 .$ g of liquid water at $100^{\circ} \mathrm{C}$ is cooled to body temperature $\left(37^{\circ} \mathrm{C}\right) ?$
(c) Why are steam burns more painful than hotwater burns?

David Collins

Numerade Educator

Problem 83

When iodine vapor hits a cold surface, iodine crystals form. Name the phase change that is the reverse of this condensation.

David Collins

Numerade Educator

Problem 84

If a 156 -g block of dry ice, $\mathrm{CO}_{2}$, is sublimed at $25^{\circ} \mathrm{C}$ and $740 \mathrm{mm} \mathrm{Hg}$, what volume does the gas occupy?

David Collins

Numerade Educator

Problem 85

Trichlorofluoromethane (Freon-11, CCl $_{3} \mathrm{F}$ ) as a spray is used to temporarily numb the skin around minor scrapes and bruises. It accomplishes this by reducing the temperature of the treated area, thereby numbing the nerve endings that perceive pain. Calculate the heat in kilocalories that can be removed from the skin by $1.00 \mathrm{mL}$ of Freon-11. The density of Freon-11 is $1.49 \mathrm{g} / \mathrm{mL}$, and its heat of vaporization is $6.42 \mathrm{kcal} / \mathrm{mol}$.

David Collins

Numerade Educator

Problem 86

Using the phase diagram of water (Figure $5-20$ ), describe the process by which you can sublime 1 g of ice at $-10^{\circ} \mathrm{C}$ and at 1 atm pressure to water vapor at the same temperature.

David Collins

Numerade Educator

Problem 87

(Chemical Connections 5 A) What happens when a person lowers the diaphragm in his or her chest cavity?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 88

(Chemical Connections $5 \mathrm{B}$ ) In carbon monoxide poisoning, the hemoglobin is incapable of transporting oxygen to the tissues. How does the oxygen get delivered to the cells when a patient is put into a hyperbaric chamber?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 89

(Chemical Connections $5 \mathrm{C}$ ) In a sphygmomanometer one listens to the first tapping sound as the constrictive pressure of the arm cuff is slowly released. What is the significance of this tapping sound?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 90

(Chemical Connections 5 D) Why is the damage by severe frostbite irreversible?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 91

(Chemical Connections 5 D) If you fill a glass bottle with water, cap it, and cool to $-10^{\circ} \mathrm{C}$, the bottle will crack. Explain.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 92

(Chemical Connections $5 \mathrm{E}$ ) In what way does supercritical $\mathrm{CO}_{2}$ have some of the properties of a gas and some of the properties of a liquid?

David Collins

Numerade Educator

Problem 93

Why is it difficult to compress a liquid or a solid?

Kyle Ukes

Numerade Educator

Problem 94

Explain in terms of the kinetic molecular theory what causes (a) the pressure of a gas and (b) the temperature of a gas.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 95

The unit of pressure most commonly used for checking the inflation of automobile and bicycle tires is pounds per square inch $\left(1 \mathrm{b} / \mathrm{in}^{2}\right),$ abbreviated psi. The conversion factor between atm and psi is 1.00 atm $=14.7$ psi. Suppose an automobile tire is filled to a pressure of 34 psi. What is the pressure in atm in the tire?

David Collins

Numerade Educator

Problem 96

The gas in an aerosol can is at a pressure of 3.0 atm at $23^{\circ} \mathrm{C}$. What will the pressure of the gas in the can be if the temperature is raised to $400^{\circ} \mathrm{C} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 97

Why do aerosol cans carry the warning "Do not incinerate"?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 98

Under certain weather conditions (just before rain), the air becomes less dense. How does this change affect the barometric pressure reading?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 99

An ideal gas occupies $387 \mathrm{mL}$ at $275 \mathrm{mm}$ Hg and $75^{\circ} \mathrm{C}$ If the pressure changes to 1.36 atm and the temperature increases to $105^{\circ} \mathrm{C}$, what is the new volume?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 100

Arrange the following solids in order of increasing expected melting points: $\mathrm{CO}_{2}(s), \mathrm{Xe}(s), \mathrm{CaO}(s)$
$\mathrm{H}_{2} \mathrm{O}(s), \mathrm{LiCl}(s),$ and $\mathrm{HCl}(s)$.

David Collins

Numerade Educator

Problem 101

On the basis of what you have learned about intermolecular forces, predict which liquid has the highest boiling point:
(a) Pentane, $\mathrm{C}_{5} \mathrm{H}_{12}$
(b) Chloroform, $\mathrm{CHCl}_{3}$
(c) Water, $\mathrm{H}_{2} \mathrm{O}$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 102

A 10 -L gas cylinder is filled with $\mathrm{N}_{2}$ to a pressure of 35 in. Hg. How many moles of $\mathrm{N}_{2}$ do you have to add to your container to raise the pressure to 60 in. $\mathrm{Hg}$ ? Assume a constant temperature of $27^{\circ} \mathrm{C}$.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 103

When filled, a typical tank for an outdoor grill contains
20. Ib of LP (liquefied petroleum) gas, the major component of which is propane, $\mathrm{C}_{3} \mathrm{H}_{8}$. For this problem, assume that propane is the only substance present.
(a) How do you account for the fact that when propane is put under pressure, it can be liquefied?
(b) How many kilograms of propane does a full tank contain?
(c) How many moles of propane does a full tank contain?
(d) If the propane in a full tank was released into a flexible container, what volume would it occupy at STP?

David Collins

Numerade Educator

Problem 104

Explain why many gases are transparent.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 105

The density of a gas is $0.00300 \mathrm{g} / \mathrm{cm}^{3}$ at $100 .^{\circ} \mathrm{C}$ and 1.00 atm. What is the mass of one mole of the gas?

Madeline Currie

Madeline Currie

Numerade Educator

Problem 106

The normal boiling point of hexane, $\mathrm{C}_{6} \mathrm{H}_{14},$ is $69^{\circ} \mathrm{C}$ and that of pentane, $\mathrm{C}_{5} \mathrm{H}_{12}$, is $36^{\circ} \mathrm{C}$. Predict which of these compounds has a higher vapor pressure at $20^{\circ} \mathrm{C}$.

Yash Ramgopal

Numerade Educator

Problem 107

If $60.0 \mathrm{g}$ of $\mathrm{NH}_{3}$ occupies $35.1 \mathrm{L}$ under a pressure of 77.2 in. Hg, what is the temperature of the gas, in $^{\circ} \mathrm{C} ?$

Yash Ramgopal

Numerade Educator

Problem 108

Water is a liquid at STP. Hydrogen sulfide, $\mathrm{H}_{2} \mathrm{S}$, a heavier molecule, is a gas under the same conditions. Explain.

Madeline Currie

Madeline Currie

Numerade Educator

Problem 109

Why does the temperature of a liquid drop as a result of evaporation?

David Collins

Numerade Educator

Problem 110

What volume of air $(21 \% \text { oxygen })$ measured at $25^{\circ} \mathrm{C}$ and 0.975 atm is required to completely oxidize 3.42 $\mathrm{g}$ of aluminum to aluminum oxide, $\mathrm{Al}_{2} \mathrm{O}_{3} ?$

Madeline Currie

Madeline Currie

Numerade Educator

Problem 111

Diving, particularly SCUBA (Self-Contained Underwater Breathing Apparatus) diving, subjects the body to increased pressure. Each $10 .$ m (approximately $33 \mathrm{ft}$ ) of water exerts an additional pressure of 1 atm on the body.
(a) What is the pressure on the body at a depth of $100 . \mathrm{ft} ?$
(b) The partial pressure of nitrogen gas in air at 1 atm is $593 \mathrm{mm}$ Hg. Assuming a SCUBA diver breathes compressed air, what is the partial pressure of nitrogen entering the lungs from a breathing tank at a depth of $100 .$ ft?
(c) The partial pressure of oxygen gas in the air at 2 atm is $158 \mathrm{mm}$ Hg. What is the partial pressure of oxygen in the air in the lungs at a depth of $100 . \mathrm{ft} ?$
(d) Why is it absolutely essential to exhale vigorously in a rapid ascent from a depth of $100 . \mathrm{ft} ?$

Rashmi Sinha

Numerade Educator

Problem 112

Consider the mixing of $3.5 \mathrm{L}$ of $\mathrm{CO}_{2}(g)$ and $1.8 \mathrm{L}$ $\operatorname{of} \mathrm{H}_{2} \mathrm{O}(g)$ at $35^{\circ} \mathrm{C}$ and $740 \mathrm{mm}$ Hg. Determine the
mass of $\mathrm{O}_{2}(g)$ that can be produced from the unbalanced reaction:
\[\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \longrightarrow \mathrm{C}_{4} \mathrm{H}_{10}(l)+\mathrm{O}_{2}(g)\]

David Collins

Numerade Educator

Problem 113

Ammonia and gaseous hydrogen chloride react to form ammonium chloride according to the following equation:
\[\mathrm{NH}_{3}(g)+\mathrm{HCl}(g) \longrightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)\]
If $4.21 \mathrm{L}$ of $\mathrm{NH}_{3}(g)$ at $27^{\circ} \mathrm{C}$ and 1.02 atm is combined with $5.35 \mathrm{L}$ of $\mathrm{HCl}(g)$ at $26^{\circ} \mathrm{C}$ and 0.998 atm, what mass of $\mathrm{NH}_{4} \mathrm{Cl}(s)$ will be generated?

David Collins

Numerade Educator

Problem 114

Carbon dioxide gas, saturated with water vapor, can be produced by the addition of aqueous acid to calcium carbonate based on the following balanced net ionic equation:
$\mathrm{CaCO}_{3}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(g)$
(a) How many moles of wet $\mathrm{CO}_{2}(\mathrm{g}),$ collected at $60 \cdot^{\circ} \mathrm{C}$ and 774 torr total pressure, are produced by the complete reaction of $10.0 \mathrm{g}$ of $\mathrm{CaCO}_{3}$ with excess acid?
(b) What volume does this wet $\mathrm{CO}_{2}$ occupy?
(c) What volume would the $\mathrm{CO}_{2}$ occupy at 774 torr if a desiccant (a chemical drying agent) were added to remove the water? The vapor pressure of water at $60 .^{\circ} \mathrm{C}$ is $149.4 \mathrm{mm} \mathrm{Hg}$.

David Collins

Numerade Educator

Problem 115

Ammonium nitrite decomposes upon heating to form nitrogen gas and water vapor according to the following unbalanced chemical reaction:
\[\mathrm{NH}_{4} \mathrm{NO}_{2}(s) \longrightarrow \mathrm{N}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\]
When a sample is decomposed in a test tube, $511 \mathrm{mL}$ of wet $\mathrm{N}_{2}(g)$ is collected over water at $26^{\circ} \mathrm{C}$ and 745 torr total pressure. How many grams of dry $\mathrm{NH}_{4} \mathrm{NO}_{2}(s)$ were initially decomposed? The vapor pressure of water at $26^{\circ} \mathrm{C}$ is 25.2 torr.

David Collins

Numerade Educator

Problem 116

How much total heat in calories is required to raise the temperature of $3.50 \mathrm{g}$ of ice at $-10.0^{\circ} \mathrm{C}$ to water vapor at $115^{\circ} \mathrm{C} ?$ Refer to Table $5-5$ for relevant data.

David Collins

Numerade Educator

Problem 117

Determine the total amount of heat lost in calories when 5.75 g of water vapor at $120 .^{\circ} \mathrm{C}$ is cooled to $-20 .^{\circ} \mathrm{C} .$ Refer to Table $5-5$ for relevant data.

David Collins

Numerade Educator

Problem 118

Isooctane, which has a chemical formula $\mathrm{C}_{8} \mathrm{H}_{18},$ is the component of gasoline from which the term octane rating derives.
(a) Write the balanced chemical equation for the combustion of isooctane.
(b) The density of isooctane is $0.792 \mathrm{g} / \mathrm{mL}$. How many $\mathrm{kg}$ of $\mathrm{CO}_{2}$ are produced each year by the annual U.S. gasoline consumption of $4.6 \times 10^{10} \mathrm{L} ?$
(c) What is the volume in liters of this $\mathrm{CO}_{2}$ at $\mathrm{STP}$ ?
(d) The chemical formula for isooctane can be represented by $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CCH}_{2} \mathrm{CH}\left(\mathrm{CH}_{3}\right)_{2}$. Draw a Lewis structure of isooctane.
(e) Another molecule with the same molecular formula is octane, which can be represented by:
When comparing isooctane and octane, one structure is observed to have a boiling point of $99^{\circ} \mathrm{C},$ while another is known to have a boiling point of $125^{\circ} \mathrm{C}$. Which substance, isooctane or octane, is expected to have the higher boiling point?
(f) Determine whether isooctane or octane is expected to have the greater vapor pressure.

David Collins

Numerade Educator

Problem 119

Consider the decomposition of solid ammonium nitrate to form gaseous dinitrogen oxide and water vapor. A 2.50 g sample of $\mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{s})$ is introduced into a 1.75 L flask and heated to $230^{\circ} \mathrm{C}$.
(a) Write the balanced chemical equation for this decomposition process.
(b) What is the partial pressure of $\mathrm{N}_{2} \mathrm{O}(\mathrm{g})$ and $\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$ produced?
(c) Determine the total gas pressure present in the flask at $230^{\circ} \mathrm{C}$
(d) Using VSEPR theory, draw three equivalent resonance structures for $\mathrm{N}_{2} \mathrm{O}(\mathrm{g})$.

David Collins

Numerade Educator

Problem 120

A 0.325 g sample of a compound containing carbon and hydrogen only occupies a volume of $193 \mathrm{mL}$ at $749 \mathrm{mm} \mathrm{Hg}$ and $26.1^{\circ} \mathrm{C}$
(a) Determine the molecular weight of this compound containing carbon and hydrogen only.
(b) Draw a possible Lewis structure for this compound.
(c) Determine the various relative bond angles associated with each central atom of this compound using VSEPR theory.
(d) Would you predict this compound to be polar or nonpolar?
(e) What types of intermolecular forces are present in a container with this compound?

David Collins

Numerade Educator