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University Physics with Modern Physics In SI Units

Hugh D Young; Roger A Freedman

Chapter 18

Thermal Properties of Matter - all with Video Answers

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Chapter Questions

02:30

Problem 1

A 20.0 L tank contains $4.86 \times 10^{-4} \mathrm{~kg}$ of helium at $18.0^{\circ} \mathrm{C}$. The molar mass of helium is $4.00 \mathrm{~g} / \mathrm{mol}$. (a) How many moles of helium are in the tank? (b) What is the pressure in the tank, in pascals and in atmospheres?

Nishant Kumar
Nishant Kumar
Numerade Educator
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Problem 2

Helium gas with a volume of $2.05 \mathrm{~L},$ under a pressure of 0.135 atm and at $37.0^{\circ} \mathrm{C}$, is warmed until both pressure and volume are doubled. (a) What is the final temperature? (b) How many grams of helium are there? The molar mass of helium is $4.00 \mathrm{~g} / \mathrm{mol}$.

Eduard Sanchez
Eduard Sanchez
Numerade Educator
04:09

Problem 3

A cylindrical tank has a tight-fitting piston that allows the volume of the tank to be changed. The tank originally contains $0.135 \mathrm{~m}^{3}$ of air at a pressure of 0.730 atm. The piston is slowly pulled out until the volume of the gas is increased to $0.370 \mathrm{~m}^{3}$. If the temperature remains constant, what is the final value of the pressure?

Aparna Shakti
Aparna Shakti
Numerade Educator
05:24

Problem 4

A $3.00 \mathrm{~L}$ tank contains air at $3.00 \mathrm{~atm}$ and $20.0^{\circ} \mathrm{C}$. The tank is sealed and cooled until the pressure is 1.00 atm. (a) What is the temperature then in degrees Celsius? Assume that the volume of the tank is constant. (b) If the temperature is kept at the value found in part (a) and the gas is compressed, what is the volume when the pressure again becomes $3.00 \mathrm{~atm} ?$

TP
Tuan Pham
University of Wisconsin - Madison
07:45

Problem 5

The discussion following Eq. (18.7) gives the constants in the van der Waals equation for $\mathrm{CO}_{2}$ gas. It also says that at STP the van der Waals equation gives only a small $(0.5 \%)$ correction in the ideal-gas equation. Consider 1 mole of $\mathrm{CO}_{2}$ gas at $T=273.0 \mathrm{~K}$ and a volume of $4.48 \times 10^{-4} \mathrm{~m}^{3}$. (a) What is the pressure of the gas calculated by the ideal-gas equation? (b) What does the van der Waals equation give for the pressure? What is the percentage difference from the ideal-gas result?

Rory Naguib
Rory Naguib
Numerade Educator
03:48

Problem 6

You have several identical balloons. You experimentally determine that a balloon will break if its volume exceeds $0.900 \mathrm{~L}$.The pressure of the gas inside the balloon equals air pressure $(1.00 \mathrm{~atm}) .(\mathrm{a})$ If the air inside the balloon is at a constant $22.0^{\circ} \mathrm{C}$ and behaves as an ideal gas, what mass of air can you blow into one of the balloons before it bursts? (b) Repeat part (a) if the gas is helium rather than air.

Averell Hause
Averell Hause
Carnegie Mellon University
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Problem 7

A Jaguar XK8 convertible has an eight-cylinder engine. At the beginning of its compression stroke, one of the cylinders contains $494 \mathrm{~cm}^{3}$ of air at atmospheric pressure $\left(1.01 \times 10^{5} \mathrm{~Pa}\right)$ and a temperature of $27.0^{\circ} \mathrm{C}$. At the end of the stroke, the air has been compressed to a volume of $46.4 \mathrm{~cm}^{3}$ and the gauge pressure has increased to $2.70 \times 10^{6} \mathrm{~Pa}$. Compute the final temperature.

Lainey Roebuck
Lainey Roebuck
Numerade Educator
06:12

Problem 8

A welder using a tank of volume $0.0750 \mathrm{~m}^{3}$ fills it with oxygen (molar mass $32.0 \mathrm{~g} / \mathrm{mol}$ ) at a gauge pressure of $3.00 \times 10^{5} \mathrm{~Pa}$ and temperature of $37.0^{\circ} \mathrm{C}$. The tank has a small leak, and in time some of the oxygen leaks out. On a day when the temperature is $22.0^{\circ} \mathrm{C},$ the gauge pressure of the oxygen in the tank is $1.80 \times 10^{5} \mathrm{~Pa}$. Find (a) the initial mass of oxygen and (b) the mass of oxygen that has leaked out.

Averell Hause
Averell Hause
Carnegie Mellon University
03:37

Problem 9

A large cylindrical tank contains $0.750 \mathrm{~m}^{3}$ of nitrogen gas at $27^{\circ} \mathrm{C}$ and $7.50 \times 10^{3} \mathrm{~Pa}$ (absolute pressure). The tank has a tight-fitting piston that allows the volume to be changed. What will be the pressure if the volume is decreased to $0.410 \mathrm{~m}^{3}$ and the temperature is increased to $157^{\circ} \mathrm{C} ?$

Shital Rijal
Shital Rijal
Numerade Educator
03:20

Problem 10

An empty cylindrical canister $1.60 \mathrm{~m}$ long and $90.0 \mathrm{~cm}$ in diameter is to be filled with pure oxygen at $28.0^{\circ} \mathrm{C}$ to store in a space station. To hold as much gas as possible, the absolute pressure of the oxygen will be 22.0 atm. The molar mass of oxygen is $32.0 \mathrm{~g} /$ mol. (a) How many moles of oxygen does this canister hold?
(b) For someone lifting this canister, by how many kilograms does this gas increase the mass to be lifted?

Khaled Yasein
Khaled Yasein
Numerade Educator
03:34

Problem 11

The gas inside a balloon will always have a pressure nearly equal to atmospheric pressure, since that is the pressure applied to the outside of the balloon. You fill a balloon with helium (a nearly ideal gas) to a volume of $0.670 \mathrm{~L}$ at $17.0^{\circ} \mathrm{C}$. What is the volume of the balloon if you cool it to the boiling point of liquid nitrogen $(77.3 \mathrm{~K})$ ?

James Kiss
James Kiss
Numerade Educator
05:04

Problem 12

An ideal gas has a density of $1.33 \times 10^{-6} \mathrm{~g} / \mathrm{cm}^{3}$ at $1.00 \times 10^{-3}$ atm and $20.0^{\circ} \mathrm{C}$. Identify the gas.

Averell Hause
Averell Hause
Carnegie Mellon University
03:04

Problem 13

If a certain amount of ideal gas occupies a volume $V$ at STP on earth, what would be its volume (in terms of $V$ ) on Venus, where the temperature is $1003^{\circ} \mathrm{C}$ and the pressure is 92 atm?

Shoukat Ali
Shoukat Ali
Other Schools
05:28

Problem 14

A diver observes a bubble of air rising from the bottom of a lake (where the absolute pressure is $3.50 \mathrm{~atm}$ ) to the surface (where the pressure is $1.00 \mathrm{~atm})$. The temperature at the bottom is $4.0^{\circ} \mathrm{C},$ and the temperature at the surface is $23.0^{\circ} \mathrm{C}$.
(a) What is the ratio of the volume of the bubble as it reaches the surface to its volume at the bottom?
(b) Would it be safe for the diver to hold his breath while ascending from the bottom of the lake to the surface? Why or why not?

Ceren Uzun
Ceren Uzun
Texas Tech University
03:16

Problem 15

How many moles of an ideal gas exert a gauge pressure of 0.876 atm in a volume of $5.43 \mathrm{~L}$ at a temperature of $22.2^{\circ} \mathrm{C} ?$

Rory Naguib
Rory Naguib
Numerade Educator
07:38

Problem 16

Three moles of an ideal gas are in a rigid cubical box with sides of length $0.170 \mathrm{~m} .$ (a) What is the force that the gas exerts on each of the six sides of the box when the gas temperature is $16.0^{\circ} \mathrm{C} ?$ (b) What is the force when the temperature of the gas is increased to $107.0^{\circ} \mathrm{C} ?$

James Kiss
James Kiss
Numerade Educator
04:42

Problem 17

(a) Calculate the mass of nitrogen present in a volume of $3000 \mathrm{~cm}^{3}$ if the gas is at $22.0^{\circ} \mathrm{C}$ and the absolute pressure of $2.00 \times 10^{-13}$ atm is a partial vacuum easily obtained in laboratories.
(b) What is the density (in $\mathrm{kg} / \mathrm{m}^{3}$ ) of the $\mathrm{N}_{2}$ ?

Rory Naguib
Rory Naguib
Numerade Educator
02:10

Problem 18

At an altitude of $11,000 \mathrm{~m}$ (a typical cruising altitude for a jet airliner), the air temperature is $-56.5^{\circ} \mathrm{C}$ and the air density is $0.364 \mathrm{~kg} / \mathrm{m}^{3}$. What is the pressure of the atmosphere at that altitude? (Note: The temperature at this altitude is not the same as at the surface of the earth, so the calculation of Example 18.4 in Section 18.1 doesn't apply.)

Khoobchandra Agrawal
Khoobchandra Agrawal
Numerade Educator
02:34

Problem 19

How many moles are in a $1.00 \mathrm{~kg}$ bottle of water? How many molecules? The molar mass of water is $18.0 \mathrm{~g} / \mathrm{mol}$.

Shital Rijal
Shital Rijal
Numerade Educator
01:24

Problem 20

A large organic molecule has a mass of $1.41 \times 10^{-21} \mathrm{~kg}$. What is the molar mass of this compound?

Rory Naguib
Rory Naguib
Numerade Educator
08:37

Problem 21

Modern vacuum pumps make it easy to attain pressures of the order of $10^{-13}$ atm in the laboratory. Consider a volume of air and treat the air as an ideal gas.
(a) At a pressure of $9.05 \times 10^{-14}$ atm and an ordinary temperature of $295.0 \mathrm{~K}$, how many molecules are present in a volume of $1.05 \mathrm{~cm}^{3} ?$ (b) How many molecules would be present at the same temperature but at 1.10 atm instead?

James Kiss
James Kiss
Numerade Educator
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Problem 22

The Lagoon Nebula (Fig. E18.22) is a cloud of hydrogen gas located 3900 light-years from the earth. The cloud is about 45 lightyears in diameter and glows because of its high temperature of $7500 \mathrm{~K}$. (The gas is raised to this temperature by the stars that lie within the nebula.) The cloud is also very thin; there are only 80 molecules per cubic centimeter. (a) Find the gas pressure (1n atmospheres) in the Lagoon Nebula. Compare it to the laboratory pressure referred to in Exercise 18.21. (b) Science-fiction films sometimes show starships being buffeted by turbulence as they fly through gas clouds such as the Lagoon Nebula. Does this seem realistic? Why or why not?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
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Problem 23

How Close Together Are Gas Molecules? Consider an ideal gas at $27^{\circ} \mathrm{C}$ and $1.00 \mathrm{~atm} .$ To get some idea how close these molecules are to each other, on the average, imagine them to be uniformly spaced, with each molecule at the center of a small cube.
(a) What is the length of an edge of each cube if adjacent cubes touch but do not overlap? (b) How does this distance compare with the diameter of a typical molecule? (c) How does their separation compare with the spacing of atoms in solids, which typically are about $0.3 \mathrm{nm}$ apart?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
04:32

Problem 24

A container with rigid walls holds $n$ moles of a monatomic ideal gas. In terms of $n$, how many moles of the gas must be removed from the container to double the pressure while also doubling the rms speed of the gas atoms?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:30

Problem 25

(a) What is the total translational kinetic energy of the air in an empty room that has dimensions $8.00 \mathrm{~m} \times 12.00 \mathrm{~m} \times 4.00 \mathrm{~m}$ if the air is treated as an ideal gas at $1.00 \mathrm{~atm} ?(\mathrm{~b})$ What is the speed of a $2000 \mathrm{~kg}$ automobile if its kinetic energy equals the translational kinetic energy calculated in part (a)?

Shital Rijal
Shital Rijal
Numerade Educator
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Problem 26

A flask contains a mixture of neon (Ne), krypton (Kr), and radon (Rn) gases. Compare (a) the average kinetic energies of the three types of atoms and (b) the root-mean-square speeds. (Hint: Appendix F shows the molar mass (in $\mathrm{g} / \mathrm{mol}$ ) of each element under the chemical symbol for that element.)

Eduard Sanchez
Eduard Sanchez
Numerade Educator
04:19

Problem 27

A container with volume $80.0 \mathrm{~cm}^{3}$ and rigid walls holds a monatomic ideal gas. To determine the number of gas atoms in the container, you measure the pressure $p_{\text {atm }}$ of the gas in atmospheres as a function of the Celsius temperature $T_{\mathrm{C}}$ of the gas. You plot $p_{\text {atm }}$ versus $T_{\mathrm{C}}$ and find that your data lie close to a straight line that has slope $1.10 \mathrm{~atm} / \mathrm{C}^{\circ} .$ What is your experimental result for the number of gas atoms?

Rory Naguib
Rory Naguib
Numerade Educator
06:19

Problem 28

A container with volume $1.65 \mathrm{~L}$ is initially evacuated. Then it is filled with $0.220 \mathrm{~g}$ of $\mathrm{N}_{2}$. Assume that the pressure of the gas is low enough for the gas to obey the ideal-gas law to a high degree of accuracy. If the root-mean-square speed of the gas molecules is $192 \mathrm{~m} / \mathrm{s}$, what is the pressure of the gas?

James Kiss
James Kiss
Numerade Educator
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Problem 29

(a) A deuteron, ${ }_{1}^{2} \mathrm{H},$ is the nucleus of a hydrogen isotope and consists of one proton and one neutron. The plasma of deuterons in a nuclear fusion reactor must be heated to about $3.07 \times 10^{8} \mathrm{~K}$. What is the rms speed of the deuterons? Is this a significant fraction of the speed of light in vacuum $\left(c=3.0 \times 10^{8} \mathrm{~m} / \mathrm{s}\right) ?(\mathrm{~b})$ What would the temperature of the plasma be if the deuterons had an rms speed equal to $9.0 \times 10^{-2} c$ ?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
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Problem 30

Martian Climate. The atmosphere of Mars is mostly $\mathrm{CO}_{2}$ (molar mass $44.0 \mathrm{~g} / \mathrm{mol}$ ) under a pressure of $650 \mathrm{~Pa}$, which we shall assume remains constant. In many places the temperature varies from $0.0^{\circ} \mathrm{C}$ in summer to $-100^{\circ} \mathrm{C}$ in winter. Over the course of a Martian year, what are the ranges of (a) the rms speeds of the $\mathrm{CO}_{2}$ molecules and (b) the density (in $\mathrm{mol} / \mathrm{m}^{3}$ ) of the atmosphere?

Eduard Sanchez
Eduard Sanchez
Numerade Educator
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Problem 31

Oxygen $\left(\mathrm{O}_{2}\right)$ has a molar mass of $32.0 \mathrm{~g} / \mathrm{mol}$. What is (a) the average translational kinetic energy of an oxygen molecule at a temperature of $300 \mathrm{~K} ;$ (b) the average value of the square of its speed; (c) the rootmean-square speed; (d) the momentum of an oxygen molecule traveling at this speed? (e) Suppose an oxygen molecule traveling at this speed bounces back and forth between opposite sides of a cubical vessel $0.18 \mathrm{~m}$ on a side. What is the average force the molecule exerts on one of the walls of the container? (Assume that the molecule's velocity is perpendicular to the two sides that it strikes.) (f) What is the average force per unit area? (g) How many oxygen molecules traveling at this speed are necessary to produce an average pressure of $1 \mathrm{~atm} ?$ (h) Compute the number of oxygen molecules that are contained in a vessel of this size at $300 \mathrm{~K}$ and atmospheric pressure. (i) Your answer for part (h) should be three times as large as the answer for part $(\mathrm{g})$. Where does this discrepancy arise?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
04:16

Problem 32

Calculate the mean free path of air molecules at $7.00 \times 10^{-13} \mathrm{~atm}$ and $296 \mathrm{~K}$. (This pressure is readily attainable in the laboratory; see Exercise $18.23 .$ ) As in Example 18.8 , model the air molecules as spheres of radius $2.0 \times 10^{-10} \mathrm{~m}$.

James Kiss
James Kiss
Numerade Educator
03:50

Problem 33

At what temperature is the root-mean-square speed of nitrogen molecules equal to the root-mean-square speed of hydrogen molecules at $20.0^{\circ} \mathrm{C} ?$ (Hint: Appendix $\mathrm{F}$ shows the molar mass (in $\mathrm{g} / \mathrm{mol}$ ) of each element under the chemical symbol for that element. The molar mass of $\mathrm{H}_{2}$ is twice the molar mass of hydrogen atoms, and similarly for $\mathrm{N}_{2}$.)

James Kiss
James Kiss
Numerade Educator
02:32

Problem 34

Smoke particles in the air typically have masses on the order of $10^{-16} \mathrm{~kg}$. The Brownian motion (rapid, irregular movement) of these particles, resulting from collisions with air molecules, can be observed with a microscope.
(a) Find the root-mean-square speed of Brownian motion for a particle with a mass of $3.00 \times 10^{-16} \mathrm{~kg}$ in air at $300 \mathrm{~K}$.
(b) Would the root-mean-square speed be different if the particle were in hydrogen gas at the same temperature? Explain.

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
07:48

Problem 35

Three moles of helium gas (molar mass $M=4.00 \mathrm{~g} / \mathrm{mol}$ ) are in a rigid container that keeps the volume of the gas constant. Initially the rms speed of the gas atoms is $900 \mathrm{~m} / \mathrm{s}$. What is the rms speed of the gas atoms after $2400 \mathrm{~J}$ of heat energy is added to the gas?

Yaqub Khan
Yaqub Khan
Numerade Educator
04:06

Problem 36

A rigid container holds 4.00 mol of a monatomic ideal gas that has temperature $300 \mathrm{~K}$. The initial pressure of the gas is $6.00 \times 10^{4} \mathrm{~Pa}$. What is the pressure after $6000 \mathrm{~J}$ of heat energy is added to the gas?

Rory Naguib
Rory Naguib
Numerade Educator
03:13

Problem 37

How much heat does it take to increase the temperature of $1.80 \mathrm{~mol}$ of an ideal gas by $50.0 \mathrm{~K}$ near room temperature if the gas is held at constant volume and is (a) diatomic;
(b) monatomic?

Shital Rijal
Shital Rijal
Numerade Educator
03:13

Problem 38

Perfectly rigid containers each hold $n$ moles of ideal gas, one being hydrogen $\left(\mathrm{H}_{2}\right)$ and the other being neon $(\mathrm{Ne})$. If it takes $300 \mathrm{~J}$ of heat to increase the temperature of the hydrogen by $2.60^{\circ} \mathrm{C},$ by how many degrees will the same amount of heat raise the temperature of the neon?

Khaled Yasein
Khaled Yasein
Numerade Educator
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Problem 39

(a) Compute the specific heat at constant volume of nitrogen $\left(\mathrm{N}_{2}\right)$ gas, and compare it with the specific heat of liquid water. The molar mass of $\mathrm{N}_{2}$ is $28.0 \mathrm{~g} / \mathrm{mol}$. (b) You warm $1.80 \mathrm{~kg}$ of water at a constant volume of $1.00 \mathrm{~L}$ from $19.0^{\circ} \mathrm{C}$ to $32.0^{\circ} \mathrm{C}$ in a kettle. For the same amount of heat, how many kilograms of $19.0^{\circ} \mathrm{C}$ air would you be able to warm to $32.0^{\circ} \mathrm{C} ?$ What volume (in liters) would this air occupy at $19.0^{\circ} \mathrm{C}$ and a pressure of 1.20 atm? Make the simplifying assumption that air is $100 \% \mathrm{~N}_{2}$.

Lainey Roebuck
Lainey Roebuck
Numerade Educator
05:52

Problem 40

(a) Calculate the specific heat at constant volume of water vapor, assuming the nonlinear triatomic molecule has three translational and three rotational degrees of freedom and that vibrational motion does not contribute. The molar mass of water is $18.0 \mathrm{~g} / \mathrm{mol}$. (b) The actual specific heat of water vapor at low pressures is about $2000 \mathrm{~J} / \mathrm{kg} \cdot \mathrm{K}$. Compare this with your calculation and comment on the actual role of vibrational motion.

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
09:02

Problem 41

For diatomic carbon dioxide $\operatorname{gas}\left(\mathrm{CO}_{2},\right.$ molar mass $44.0 \mathrm{~g} / \mathrm{mol}$ ) at $T=300 \mathrm{~K},$ calculate (a) the most probable speed $v_{\mathrm{mp}} ;$ (b) the average speed $v_{\mathrm{av}} ;$ (c) the root-mean-square speed $v_{\mathrm{rms}}$

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
06:38

Problem 42

For a gas of nitrogen molecules $\left(\mathrm{N}_{2}\right),$ what must the temperature be if $94.7 \%$ of all the molecules have speeds less than (a) $1500 \mathrm{~m} / \mathrm{s} ;$
(b) $1000 \mathrm{~m} / \mathrm{s} ;$ (c) $500 \mathrm{~m} / \mathrm{s}$ ? Use Table 18.2. The molar mass of $\mathrm{N}_{2}$ is $28.0 \mathrm{~g} / \mathrm{mol}$

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
04:12

Problem 43

The speed of sound for an ideal gas is given by $v=\sqrt{\gamma R T / M}$ [Eq. (16.10)]. We'll see in Chapter 19 that for a monatomic ideal gas, $\gamma=1.67$. (a) What is the ratio $v_{\mathrm{rms}} / v ?$ (b) The average speed $v_{\mathrm{av}}$ of the gas atoms is given by Eq. (18.35). What is the ratio $v_{\mathrm{av}} / v ?$

Rory Naguib
Rory Naguib
Numerade Educator
02:51

Problem 44

In 0.0345 mol of a monatomic ideal gas, how many of the atoms have speeds that are within $20 \%$ of the rms speed? (Use Table 18.2.)

Hubert Agamasu
Hubert Agamasu
Numerade Educator
04:24

Problem 45

Solid water (ice) is slowly warmed from a very low temperature. (a) What minimum external pressure $p_{1}$ must be applied to the solid if a melting phase transition is to be observed? Describe the sequence of phase transitions that occur if the applied pressure $p$ is such that $p<p_{1}$. (b) Above a certain maximum pressure $p_{2}$, no boiling transition is observed. What is this pressure? Describe the sequence of phase transitions that occur if $p_{1}<p<p_{2}$.

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
02:09

Problem 46

Meteorology. The vapor pressure is the pressure of the vapor phase of a substance when it is in equilibrium with the solid or liquid phase of the substance. The relative humidity is the partial pressure of water vapor in the air divided by the vapor pressure of water at that same temperature, expressed as a percentage. The air is saturated when the humidity is $100 \%$.
(a) The vapor pressure of water at $20.0^{\circ} \mathrm{C}$ is $2.34 \times 10^{3} \mathrm{~Pa}$. If the air temperature is $20.0^{\circ} \mathrm{C}$ and the relative humidity is $60 \%,$ what is the partial pressure of water vapor in the atmosphere (that is, the pressure due to water vapor alone)? (b) Under the conditions of part (a), what is the mass of water in $1.00 \mathrm{~m}^{3}$ of air? (The molar mass of water is $18.0 \mathrm{~g} / \mathrm{mol}$. Assume that water vapor can be treated as an ideal gas.)

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
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Problem 47

Imagine the sound made when a latex balloon with a diameter of $30 \mathrm{~cm}$ pops $2 \mathrm{~m}$ from your ear. Estimate the sound intensity level in decibels, using Table 16.2 as a guide. (a) Assuming the duration of the popping event was $100 \mathrm{~ms}$, use the intensity of the popping sound to determine the average power of the pop and the energy released in the pop. This provides an estimate of the energy stored in the balloon prior to the pop. (b) Let $T$ be the ratio of the energy stored in the stretched balloon to its surface area. Use your estimate of the stored energy and the size of the balloon to estimate the value of $T$. (c) The gauge pressure of a latex balloon depends on $T$ and radius $R$ according to $p_{\text {gauge }}=T / R$. Use this information to estimate the gauge pressure in the balloon.

Lainey Roebuck
Lainey Roebuck
Numerade Educator
06:39

Problem 48

A physics lecture room at $1.00 \mathrm{~atm}$ and $27.0^{\circ} \mathrm{C}$ has a volume of $216 \mathrm{~m}^{3}$. (a) Use the ideal-gas law to estimate the number of air molecules in the room. Assume that all of the air is $\mathrm{N}_{2}$. Calculate
(b) the particle density- that is, the number of $\mathrm{N}_{2}$ molecules per cubic centimeter-and (c) the mass of the air in the room.

Averell Hause
Averell Hause
Carnegie Mellon University
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Problem 49

The Effect of Altitude on the Lungs. (a) Calculate the change in air pressure you will experience if you climb a $1050 \mathrm{~m}$ mountain, assuming that the temperature and air density do not change over this distance and that they were $22^{\circ} \mathrm{C}$ and $1.2 \mathrm{~kg} / \mathrm{m}^{3}$, respectively, at the bottom of the mountain. (Note: The result of Example 18.4 doesn't apply, since the expression derived in that example accounts for the variation of air density with altitude and we are told to ignore that here.) (b) If you took a $0.50 \mathrm{~L}$ breath at the foot of the mountain and managed to hold it until you reached the top, what would be the volume of this breath when you exhaled it there?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
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Problem 50

Decompression sickness. If deep-sea divers rise to the surface too quickly, nitrogen bubbles in their blood can expand and prove fatal. This phenomenon is known as decompression sickness (DCS, also known as the bends). If a scuba diver rises quickly from a depth of $25 \mathrm{~m}$ in Lake Baikal in Russia (which is fresh water), what will be the volume at the surface of an $\mathrm{N}_{2}$ bubble that occupied $1.0 \mathrm{~mm}^{3}$ in his blood at the lower depth? Does it seem that this difference is large enough to be a problem? (Assume that the pressure difference is due to only the changing water pressure, not to any temperature difference. This assumption is reasonable, since we are warm-blooded creatures.)

Lainey Roebuck
Lainey Roebuck
Numerade Educator
06:02

Problem 51

A hot-air balloon stays aloft because hot air at atmospheric pressure is less dense than cooler air at the same pressure. If the volume of the balloon is $500.0 \mathrm{~m}^{3}$ and the surrounding air is at $15.0^{\circ} \mathrm{C}$, what must the temperature of the air in the balloon be for it to lift a total load of $290 \mathrm{~kg}$ (in addition to the mass of the hot air)? The density of air at $15.0^{\circ} \mathrm{C}$ and atmospheric pressure is $1.23 \mathrm{~kg} / \mathrm{m}^{3}$.

Shital Rijal
Shital Rijal
Numerade Educator
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Problem 52

In an evacuated enclosure, a vertical cylindrical tank of diameter $D$ is sealed by a $3.00 \mathrm{~kg}$ circular disk that can move up and down without friction. Beneath the disk is a quantity of ideal gas at temperature $T$ in the cylinder (Fig. P18.52). Initially the disk is at rest at a distance of $h=4.00 \mathrm{~m}$ above the bottom of the tank.
When a lead brick of mass $9.00 \mathrm{~kg}$ is gently placed on the disk, the disk moves downward. If the temperature of the gas is kept constant and no gas escapes from the tank, what distance

Lainey Roebuck
Lainey Roebuck
Numerade Educator
05:43

Problem 53

A cylinder $1.00 \mathrm{~m}$ tall with inside diameter $0.120 \mathrm{~m}$ is used to hold propane gas (molar mass $44.1 \mathrm{~g} / \mathrm{mol}$ ) for use in a barbecue. It is initially filled with gas until the gauge pressure is $1.30 \times 10^{6} \mathrm{~Pa}$ at $22.0^{\circ} \mathrm{C}$. The temperature of the gas remains constant as it is partially emptied out of the tank, until the gauge pressure is $3.40 \times 10^{5} \mathrm{~Pa}$. Calculate the mass of propane that has been used.

Shital Rijal
Shital Rijal
Numerade Educator
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Problem 54

Submarine rescue. During a test dive in 1939 , prior to being accepted by the U.S. Navy, the submarine Squalus sank at a point where the depth of water was $73.0 \mathrm{~m}$. The temperature was $27.0^{\circ} \mathrm{C}$ at the surface and $7.0^{\circ} \mathrm{C}$ at the bottom. The density of seawater is $1030 \mathrm{~kg} / \mathrm{m}^{3}$.
(a) A diving bell was used to rescue 33 trapped crewmen from the Squalus in what is, to this day, the only successful submarine rescue operation. The diving bell was in the form of a circular cylinder $2.30 \mathrm{~m}$ high, open at the bottom and closed at the top. When the diving bell was lowered to the bottom of the sea, to what height did water rise within the diving bell? (Hint: Ignore the relatively small variation in water pressure between the bottom of the bell and the surface of the water within the bell.) (b) At what gauge pressure must compressed air have been supplied to the bell while on the bottom to expel all the water from it?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
12:31

Problem 55

A parcel of air over a campfire feels an upward buoyant force because the heated air is less dense than the surrounding air. By estimating the acceleration of the air immediately above a fire, one can estimate the fire's temperature. The mass of a volume $V$ of air is $n M_{\text {air }}$, where $n$ is the number of moles of air molecules in the volume and $M_{\text {air }}$ is the molar mass of air. The net upward force on a parcel of air above a fire is roughly given by $\left(m_{\text {out }}-m_{\text {in }}\right) g,$ where $m_{\text {out }}$ is the mass of a volume of ambient air and $m_{\text {in }}$ is the mass of a similar volume of air in the hot zone. (a) Use the ideal-gas law, along with the knowledge that the pressure of the air above the fire is the same as that of the ambient air, to derive an expression for the acceleration $a$ of an air parcel as a function of $\left(T_{\text {out }} / T_{\text {in }}\right),$ where $T_{\text {in }}$ is the absolute temperature of the air above the fire and $T_{\text {out }}$ is the absolute temperature of the ambient air. (b) Rearrange your formula from part (a) to obtain an expression for $T_{\text {in }}$ as a function of $T_{\text {out }}$ and $a$.
(c) Based on your experience with campfires, estimate the acceleration of the air above the fire by comparing in your mind the upward trajectory of sparks with the acceleration of falling objects. Thus you can estimate $a$ as a multiple of $g$. (d) Assuming an ambient temperature of $15^{\circ} \mathrm{C}$ use your formula and your estimate of $a$ to estimate the temperature of the fire.

Hubert Agamasu
Hubert Agamasu
Numerade Educator
04:40

Problem 56

Pressure on Venus. At the surface of Venus the average temperature is a balmy $460^{\circ} \mathrm{C}$ due to the greenhouse effect (global warming!), the pressure is 92 earth-atmospheres, and the acceleration due to gravity is $0.894 g_{\text {earth }}$. The atmosphere is nearly all $\mathrm{CO}_{2}$ (molar mass $44.0 \mathrm{~g} / \mathrm{mol}$ ), and the temperature remains remarkably constant. Assume that the temperature does not change with altitude.
(a) What is the atmospheric pressure $1.00 \mathrm{~km}$ above the surface of Venus? Express your answer in Venus-atmospheres and earth-atmospheres.
(b) What is the root-mean-square speed of the $\mathrm{CO}_{2}$ molecules at the surface of Venus and at an altitude of $1.00 \mathrm{~km} ?$

Mirza  Aslam Beig
Mirza Aslam Beig
Numerade Educator
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Problem 57

A cylindrical diving bell has a radius of $750 \mathrm{~cm}$ and a height of $2.50 \mathrm{~m}$. The bell includes a top compartment that holds an undersea adventurer. A bottom compartment separated from the top by a sturdy grating holds a tank of compressed air with a valve to release air into the bell, a second valve that can release air from the bell into the sea, a third valve that regulates the entry of seawater for ballast, a pump that removes the ballast to increase buoyancy, and an electric heater that maintains a constant temperature of $20.0^{\circ} \mathrm{C}$. The total mass of the bell and all of its apparatuses is $4350 \mathrm{~kg}$. The density of seawater is $1025 \mathrm{~kg} / \mathrm{m}^{3}$. (a) An $80.0 \mathrm{~kg}$ adventurer enters the bell. How many liters of seawater should be moved into the bell so that it is neutrally buoyant? (b) By carefully regulating ballast, the bell is made to descend into the sea at a rate of $1.0 \mathrm{~m} / \mathrm{s}$. Compressed air is released from the tank to raise the pressure in the bell to match the pressure of the seawater outside the bell. As the bell descends, at what rate should air be released through the first valve? (Hint: Derive an expression for the number of moles of air in the bell $n$ as a function of depth $y ;$ then differentiate this to obtain $d n / d t$ as a function of $d y / d t .$ ) (c) If the compressed air tank is a fully loaded, specially designed, $17 \mathrm{~m}^{3}$ tank, which means it contains that volume of air at standard temperature and pressure ( $0^{\circ} \mathrm{C}$ and $\left.1 \mathrm{~atm}\right)$, how deep can the bell descend?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
05:16

Problem 58

A flask with a volume of $1.50 \mathrm{~L},$ provided with a stopcock, contains ethane gas $\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)$ at $300 \mathrm{~K}$ and atmospheric pressure $\left(1.013 \times 10^{5} \mathrm{~Pa}\right)$. The molar mass of ethane is $30.1 \mathrm{~g} / \mathrm{mol}$. The system is warmed to a temperature of $550 \mathrm{~K},$ with the stopcock open to the atmosphere. The stopcock is then closed, and the flask is cooled to its original temperature. (a) What is the final pressure of the ethane in the flask? (b) How many grams of ethane remain in the flask?

Averell Hause
Averell Hause
Carnegie Mellon University
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Problem 59

A balloon of volume $740 \mathrm{~m}^{3}$ is to be filled with hydrogen at atmospheric pressure $\left(1.01 \times 10^{5} \mathrm{~Pa}\right) .$ (a) If the hydrogen is stored in cylinders with volumes of $1.94 \mathrm{~m}^{3}$ at a gauge pressure of $1.19 \times 10^{6} \mathrm{~Pa}$, how many cylinders are required? Assume that the temperature of the hydrogen remains constant. (b) What is the total weight (in addition to the weight of the gas) that can be supported by the balloon if both the gas in the balloon and the surrounding air are at $15.0^{\circ} \mathrm{C} ?$ The molar mass of hydrogen $\left(\mathrm{H}_{2}\right)$ is $2.02 \mathrm{~g} / \mathrm{mol}$. The density of air at $15.0^{\circ} \mathrm{C}$ and atmospheric pressure is $1.23 \mathrm{~kg} / \mathrm{m}^{3} .$ See Chapter 12 for a discussion of buoyancy.
(c) What weight could be supported if the balloon were filled with helium (molar mass $4.00 \mathrm{~g} / \mathrm{mol}$ ) instead of hydrogen, again at $15.0^{\circ} \mathrm{C} ?$

Lainey Roebuck
Lainey Roebuck
Numerade Educator
07:56

Problem 60

A vertical cylindrical tank contains 1.85 mol of an ideal gas under a pressure of 0.550 atm at $22.0^{\circ} \mathrm{C}$. The round part of the tank has a radius of $10.0 \mathrm{~cm}$, and the gas is supporting a piston that can move up and down in the cylinder without friction. There is a vacuum above the piston.
(a) What is the mass of this piston?
(b) How tall is the column of gas that is supporting the piston?

James Kiss
James Kiss
Numerade Educator
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Problem 61

A large tank of water has a hose connected to it (Fig. P18.61). The tank is sealed at the top and has compressed air between the water surface and the top. When the water height $h$ has the value $3.50 \mathrm{~m}$, the absolute pressure $p$ of the compressed air is $4.20 \times 10^{5} \mathrm{~Pa}$. Assume that the air
above the water expands at constant temperature, and take the atmospheric pressure to be $1.00 \times 10^{\circ} \mathrm{Pa}$.
(a) What is the speed with which water flows out of the hose when $h=3.50 \mathrm{~m} ?$ (b) As water flows out of the tank, $h$ decreases. Calculate the speed of flow for $h=3.00 \mathrm{~m}$ and for $h=2.00 \mathrm{~m}$.
(c) At what value of $h$ does the flow stop?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
08:02

Problem 62

A light, plastic sphere with mass $m=9.00 \mathrm{~g}$ and density $\rho=4.00 \mathrm{~kg} / \mathrm{m}^{3}$ is suspended in air by thread of negligible mass.
(a) What is the tension $T$ in the thread if the air is at $5.00^{\circ} \mathrm{C}$ and $p=1.00$ atm? The molar mass of air is $28.8 \mathrm{~g} / \mathrm{mol}$.
(b) How much does the tension in the thread change if the temperature of the gas is increased to $35.0^{\circ} \mathrm{C} ?$ Ignore the change in volume of the plastic sphere when the temperature is changed.

Averell Hause
Averell Hause
Carnegie Mellon University
02:42

Problem 63

How Many Atoms Are You? Estimate the number of atoms in the body of a $50 \mathrm{~kg}$ physics student. Note that the human body is mostly water, which has molar mass $18.0 \mathrm{~g} / \mathrm{mol}$, and that each water molecule contains three atoms.

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
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Problem 64

A person at rest inhales $0.55 \mathrm{~L}$ of air with each breath at a pressure of 1.00 atm and a temperature of $21.0^{\circ} \mathrm{C}$. The inhaled air is $21.0 \%$ oxygen. (a) How many oxygen molecules does this person inhale with each breath? (b) Suppose this person is now resting at an elevation of $2100 \mathrm{~m}$ but the temperature is still $21.0^{\circ} \mathrm{C}$. Assuming that the oxygen percentage and volume per inhalation are the same as stated above, how many oxygen molecules does this person now inhale with each breath? (c) Given that the body still requires the same number of oxygen molecules per second as at sea level to maintain its functions, explain why some people report "shortness of breath" at high elevations.

Lainey Roebuck
Lainey Roebuck
Numerade Educator
07:19

Problem 65

You blow up a spherical balloon to a diameter of $50.0 \mathrm{~cm}$ until the absolute pressure inside is 1.25 atm and the temperature is $22.0^{\circ} \mathrm{C}$. Assume that all the gas is $\mathrm{N}_{2}$, of molar mass $28.0 \mathrm{~g} / \mathrm{mol}$.
(a) Find the mass of a single $\mathrm{N}_{2}$ molecule.
(b) How much translational kinetic energy does an average $\mathrm{N}_{2}$ molecule have? (c) How many $\mathrm{N}_{2}$ molecules are in this balloon? (d) What is the total translational kinetic energy of all the molecules in the balloon?

Shital Rijal
Shital Rijal
Numerade Educator
03:29

Problem 66

The size of an oxygen molecule is about $2.0 \times 10^{-10} \mathrm{~m} .$ Make a rough estimate of the pressure at which the finite volume of the molecules should cause noticeable deviations from ideal-gas behavior at ordinary temperatures $(T=300 \mathrm{~K})$.

Hubert Agamasu
Hubert Agamasu
Numerade Educator
16:08

Problem 67

The Lennard-Jones Potential. A commonly used potential-energy function for the interaction of two molecules (see Fig. 18.8 ) is the Lennard-Jones $6-12$ potential:
$$
U(r)=U_{0}\left[\left(\frac{R_{0}}{r}\right)^{12}-2\left(\frac{R_{0}}{r}\right)^{6}\right]
$$
where $r$ is the distance between the centers of the molecules and $U_{0}$ and $R_{0}$ are positive constants. The corresponding force $F(r)$ is given in Eq. (14.26). (a) Graph $U(r)$ and $F(r)$ versus $r$. (b) Let $r_{1}$ be the value of $r$ at which $U(r)=0,$ and let $r_{2}$ be the value of $r$ at which $F(r)=0 .$ Show the locations of $r_{1}$ and $r_{2}$ on your graphs of $U(r)$ and $F(r) .$ Which of these values represents the equilibrium separation between the molecules? (c) Find the values of $r_{1}$ and $r_{2}$ in terms of $R_{0}$, and find the ratio $r_{1} / r_{2} .$ (d) If the molecules are located a distance $r_{2}$ apart [as calculated in part (c)], how much work must be done to pull them apart so that $r \rightarrow \infty$ ?

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
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Problem 68

(a) What is the total random translational kinetic energy of $4.80 \mathrm{~L}$ of hydrogen gas (molar mass $2.016 \mathrm{~g} / \mathrm{mol}$ ) with pressure $1.03 \times 10^{5} \mathrm{~Pa}$ and temperature $305 \mathrm{~K} ?$ (Hint: Use the procedure of Problem 18.65 as a guide.) (b) If the tank containing the gas is placed on a swift jet moving at $297.0 \mathrm{~m} / \mathrm{s}$, by what percentage is the total kinetic energy of the gas increased?
(c) Since the kinetic energy of the gas molecules is greater when it is on the jet, does this mean that its temperature has gone up? Explain.

Lainey Roebuck
Lainey Roebuck
Numerade Educator
03:24

Problem 69

It is possible to make crystalline solids that are only one layer of atoms thick. Such "two-dimensional" crystals can be created by depositing atoms on a very flat surface. (a) If the atoms in such a twodimensional crystal can move only within the plane of the crystal, what will be its molar heat capacity near room temperature? Give your answer as a multiple of $R$ and in $\mathrm{J} / \mathrm{mol} \cdot \mathrm{K} .$ (b) At very low temperatures, will the molar heat capacity of a two-dimensional crystal be greater than, less than, or equal to the result you found in part (a)? Explain why.

Hubert Agamasu
Hubert Agamasu
Numerade Educator
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Problem 70

Hydrogen on the Sun. The surface of the sun has a temperature of about $5800 \mathrm{~K}$ and consists largely of hydrogen atoms. (a) Find the rms speed of a hydrogen atom at this temperature. (The mass of a single hydrogen atom is $1.67 \times 10^{-27} \mathrm{~kg} .$ ) (b) The escape speed for a particle to leave the gravitational influence of the sun is given by $(2 G M / R)^{1 / 2}$, where $M$ is the sun's mass, $R$ its radius, and $G$ the gravitational constant (see Example 13.5 of Section 13.3). Use the data given at the back of the book to calculate this escape speed.
(c) Can appreciable quantities of hydrogen escape from the sun? Can any hydrogen escape? Explain.

Lainey Roebuck
Lainey Roebuck
Numerade Educator
14:00

Problem 71

(a) Show that a projectile with mass $m$ can "escape" from the surface of a planet if it is launched vertically upward with a kinetic energy greater than $m g R_{\mathrm{p}},$ where $g$ is the acceleration due to gravity at the planet's surface and $R_{\mathrm{p}}$ is the planet's radius. Ignore air resistance. (See Problem $18.70 .$ ) (b) If the planet in question is the earth, at what temperature does the average translational kinetic energy of a nitrogen molecule (molar mass $28.0 \mathrm{~g} / \mathrm{mol}$ ) equal that required to escape? What about a hydrogen molecule (molar mass $2.02 \mathrm{~g} / \mathrm{mol}$ )? (c) Repeat part (b) for the moon, for which $g=1.63 \mathrm{~m} / \mathrm{s}^{2}$ and $R_{\mathrm{p}}=1740 \mathrm{~km}$.
(d) While the earth and the moon have similar average surface temperatures, the moon has essentially no atmosphere. Use your results from parts $(\mathrm{b})$ and $(\mathrm{c})$ to explain why.

Keshav Singh
Keshav Singh
Numerade Educator
02:50

Problem 72

Helium gas is in a cylinder that has rigid walls. If the pressure of the gas is $2.00 \mathrm{~atm},$ then the root-mean-square speed of the helium atoms is $v_{\mathrm{rms}}=176 \mathrm{~m} / \mathrm{s}$. By how much (in atmospheres) must the pressure be increased to increase the $v_{\mathrm{rms}}$ of the He atoms by $100 \mathrm{~m} / \mathrm{s}$ ? Ignore any change in the volume of the cylinder.

Mirza  Aslam Beig
Mirza Aslam Beig
Numerade Educator
07:05

Problem 73

Calculate the integral in Eq. (18.31), $\int_{0}^{\infty} v^{2} f(v) d v$, and compare this result to $\left(v^{2}\right)_{\text {av }}$ as given by Eq. (18.16). (Hint: You may use the tabulated integral
$$
\int_{0}^{\infty} x^{2 n} e^{-\alpha x^{2}} d x=\frac{1 \cdot 3 \cdot 5 \cdot \cdots(2 n-1)}{2^{n+1} \alpha^{n}} \sqrt{\frac{\pi}{\alpha}}
$$
where $n$ is a positive integer and $\alpha$ is a positive constant.)

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
06:06

Problem 74

(a) Calculate the total rotational kinetic energy of the molecules in $1.00 \mathrm{~mol}$ of a diatomic gas at $300 \mathrm{~K}$.
(b) Calculate the moment of inertia of an oxygen molecule $\left(\mathrm{O}_{2}\right)$ for rotation about either the $y$ - or $z$ -axis shown in Fig. $18.18 \mathrm{~b}$. Treat the molecule as two massive points (representing the oxygen atoms) separated by a distance of $1.21 \times 10^{-10} \mathrm{~m} .$ The molar mass of oxygen atoms is $16.0 \mathrm{~g} / \mathrm{mol}$.
(c) Find the rms angular velocity of rotation of an oxygen molecule about either the $y$ - or $z$ -axis shown in Fig. $18.18 \mathrm{~b}$. How does your answer compare to the angular velocity of a typical piece of rapidly rotating machinery $(10,000 \mathrm{rev} / \mathrm{min}) ?$

Dading Chen
Dading Chen
Numerade Educator
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Problem 75

(a) Explain why in a gas of $N$ molecules, the number of molecules having speeds in the finite interval $v$ to $v+\Delta v$ is $\Delta N=N \int_{v}^{v+\Delta v} f(v) d v$. (b) If $\Delta v$ is small, then $f(v)$
is approximately constant over the interval and $\Delta N \approx N f(v) \Delta v$. For oxygen gas $\left(\mathrm{O}_{2},\right.$ molar mass $\left.32.0 \mathrm{~g} / \mathrm{mol}\right)$ at $T=294 \mathrm{~K},$ use this approximation to calculate the number of molecules with speeds within $\Delta v=13 \mathrm{~m} / \mathrm{s}$ of $v_{\mathrm{mp}} .$ Express your answer as a multiple of $N$.
(c) Repeat part (b) for speeds within $\Delta v=13 \mathrm{~m} / \mathrm{s}$ of $7 v_{\mathrm{mp}}$.
(d) Repeat parts (b) and (c) for a temperature of $588 \mathrm{~K}$. (e) Repeat parts (b) and (c) for a temperature of $147 \mathrm{~K}$. (f) What do your results tell you about the shape of the distribution as a function of temperature? Do your conclusions agree with what is shown in Fig. $18.23 ?$

Lainey Roebuck
Lainey Roebuck
Numerade Educator
08:32

Problem 76

Calculate the integral in Eq. $(18.30), \int_{0}^{\infty} v f(v) d v,$ and compare this result to $v_{\text {av }}$ as given by Eq. (18.35). (Hint: Make the change of variable $v^{2}=x$ and use the tabulated integral
$$
\int_{0}^{\infty} x^{n} e^{-\alpha x} d x=\frac{n !}{\alpha^{n+1}}
$$
where $n$ is a positive integer and $\alpha$ is a positive constant.

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
14:25

Problem 77

Oscillations of a Piston. A vertical cylinder of radius $r$ contains an ideal gas and is fitted with a piston of mass $m$ that is free to move (Fig. P18.77). The piston and the walls of the cylinder are frictionless, and the entire cylinder is placed in a constant-temperature bath. The outside air pressure is $p_{0}$. In equilibrium, the piston sits at a height $h$ above the bottom of the cylinder. (a) Find the absolute pressure of the gas trapped below the piston when in equilibrium. (b) The piston is pulled up by a small distance and released. Find the net force acting on the piston when its base is a distance $h+y$ above the bottom of the cylinder, where $y \ll h .$ (c) After the piston is displaced from equilibrium and released, it oscillates up and down. Find the frequency of these small oscillations. If the displacement is not small, are the oscillations simple harmonic? How can you tell?

Linda Winkler
Linda Winkler
Numerade Educator
07:19

Problem 78

A steel cylinder with rigid walls is evacuated to a high degree of vacuum; you then put a small amount of helium into the cylinder. The cylinder has a pressure gauge that measures the pressure of the gas inside the cylinder. You place the cylinder in various temperature environments, wait for thermal equilibrium to be established, and then measure the pressure of the gas. You obtain these results:

(a) Recall (Chapter 17 ) that absolute zero is the temperature at which the pressure of an ideal gas becomes zero. Use the data in the table to calculate the value of absolute zero in ${ }^{\circ} \mathrm{C}$. Assume that the pressure of the gas is low enough for it to be treated as an ideal gas, and ignore the change in volume of the cylinder as its temperature is changed. (b) Use the coefficient of volume expansion for steel in Table 17.2 to calculate the percentage change in the volume of the cylinder between the lowest and highest temperatures in the table. Is it accurate to ignore the volume change of the cylinder as the temperature changes? Justify your answer.

Averell Hause
Averell Hause
Carnegie Mellon University
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Problem 79

DATA The Dew Point and Clouds. The vapor pressure of water (see Exercise 18.46 ) decreases as the temperature decreases. The table lists the vapor pressure of water at various temperatures:
If the amount of water vapor in the air is kept constant as the air is cooled, the dew point temperature is reached, at which the partial pressure and vapor pressure coincide and the vapor is saturated. If the air is cooled further, the vapor condenses to liquid until the partial pressure again equals the vapor pressure at that temperature. The temperature in a room is $30.0^{\circ} \mathrm{C}$.
(a) A meteorologist cools a metal can by gradually adding cold water. When the can's temperature reaches $16.0^{\circ} \mathrm{C}$, water droplets form on its outside surface. What is the relative humidity of the $30.0^{\circ} \mathrm{C}$ air in the room? On a spring day in the midwestern United States, the air temperature at the surface is $28.0^{\circ} \mathrm{C}$. Puffy cumulus clouds form at an altitude where the air temperature equals the dew point. If the air temperature decreases with altitude at a rate of $0.6 \mathrm{C}^{\circ} / 100 \mathrm{~m}$, at approximately what height above the ground will clouds form if the relative humidity at the surface is
(b) $35 \% ;$ (c) $80 \%$ ?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
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Problem 80

The statistical quantities "average value" and "rootmean-square value" can be applied to any distribution. Figure $\mathbf{P} 18.80$ shows the scores of a class of 150 students on a 100 point quiz.
(a) Find the average score for the class.
(b) Find the rms score for the class.
(c) Which is higher: the average score or the rms score? Why?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
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Problem 81

We can crudely model a nitrogen molecule as a pair of small balls, each with the mass of a nitrogen atom, $2.3 \times 10^{-26} \mathrm{~kg}$, attached by a rigid massless rod with length $d=2 r=188 \mathrm{pm}$.
(a) What is the moment of inertia of this molecule with respect to an axis passing through the midpoint and perpendicular to the molecular axis? (b) Consider air at 1 atm pressure and $20.0^{\circ} \mathrm{C}$ temperature. Suppose two nitrogen molecules with rms speeds $v_{\mathrm{i}}$ have an elastic collision such that only one nitrogen atom in one molecule collides with one nitrogen atom in the other molecule in the manner depicted in Fig. P18.81. Write equations for the conservation of energy and the conservation of angular momentum, in terms of $r, v_{i}, v_{f},$ and $\omega,$ where $v_{f}$ and $\omega$ are, respectively, the center-of-mass speed and the angular speed of either molecule after the collision. (c) Solve these equations for $v_{\mathrm{f}}$ and $\omega$ in terms of $v_{\mathrm{i}}$ and $r .$ Note that $\omega \neq 0$ after the collision. (d) Using $v_{\mathrm{i}}=v_{\mathrm{rms}}$ for the conditions specified above, what is the frequency of rotation?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
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Problem 82

A pneumatic lift consists of a vertical cylinder with a radius of $10.0 \mathrm{~cm} .$ A movable piston slides within the cylinder at its upper end and supports a platform on which loads are placed. An intake valve allows compressed air from a tank to enter the cylinder, and an exhaust valve allows air to be removed from the cylinder. In either case the rate of air transfer is sufficiently low that the temperature in the cylinder remains constant. When neither valve is activated, the cylinder is airtight. The piston and platform together have a mass of $50.0 \mathrm{~kg},$ the temperature is $20.0^{\circ} \mathrm{C},$ and the pressure outside the cylinder is 1.00 atm. (a) There is 1.00 mol of air in the cylinder and no load on the platform. What is the height $h$ between the bottom of the piston and the bottom of the cylinder? (b) A $200 \mathrm{~kg}$ load is placed on the platform. By what distance does the platform drop?
(c) The intake valve is activated and compressed air enters the cylinder so that the platform moves back to its original height. How many moles of air were introduced? (d) How many more moles of air should be introduced so that the platform rises $2.00 \mathrm{~m}$ above its original height?
(e) At what rate should this air be introduced, in $\mathrm{mmol} / \mathrm{s}$, so that the platform rises at a rate of $10.0 \mathrm{~cm} / \mathrm{s}$ ?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
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Problem 83

Dark Nebulae and the Interstellar Medium. The dark area in Fig. $\mathbf{P} 18.83$ that appears devoid of stars is a dark nebula, a cold gas cloud in interstellar space that contains enough material to block out light from the stars behind it. A typical dark nebula is about 20 light-years in diameter and contains about 50 hydrogen atoms per cubic centimeter (monatomic hydrogen, $n o t \mathrm{H}_{2}$ ) at about $20 \mathrm{~K}$. (A lightyear is the distance light travels in vacuum in one year and is equal to $9.46 \times 10^{15} \mathrm{~m} .$ ) (a) Estimate the mean free path for a hydrogen atom in a dark nebula. The radius of a hydrogen atom is $5.0 \times 10^{-11} \mathrm{~m}$.
(b) Estimate the rms speed of a hydrogen atom and the mean free time (the average time between collisions for a given atom). Based on this result, do you think that atomic collisions, such as those leading to $\mathrm{H}_{2}$ molecule formation, are very important in determining the composition of the nebula? (c) Estimate the pressure inside a dark nebula. (d) Compare the rms speed of a hydrogen atom to the escape speed at the surface of the nebula (assumed spherical). If the space around the nebula were a vacuum, would such a cloud be stable or would it tend to evaporate?
(e) The stability of dark nebulae is explained by the presence of the interstellar medium (ISM), an even thinner gas that permeates space and in which the dark nebulae are embedded. Show that for dark nebulae to be in equilibrium with the ISM, the numbers of atoms per volume $(N / V)$ and the temperatures $(T)$ of dark nebulae and the ISM must be related by
$$
\frac{(N / V)_{\text {nebula }}}{(N / V)_{\text {ISM }}}=\frac{T_{\text {ISM }}}{T_{\text {nebula }}}
$$
(f) In the vicinity of the sun, the ISM contains about 1 hydrogen atom per $200 \mathrm{~cm}^{3}$. Estimate the temperature of the ISM in the vicinity of the sun. Compare to the temperature of the sun's surface, about $5800 \mathrm{~K}$. Would a spacecraft coasting through interstellar space burn up? Why or why not?

Lainey Roebuck
Lainey Roebuck
Numerade Educator
05:35

Problem 84

Earth's Atmosphere. In the troposphere, the part of the atmosphere that extends from earth's surface to an altitude of about $11 \mathrm{~km},$ the temperature is not uniform but decreases with increasing elevation. (a) Show that if the temperature variation is approximated by the linear relationship
$$
T=T_{0}-\alpha y
$$
where $T_{0}$ is the temperature at the earth's surface and $T$ is the temperature at height $y$, the pressure $p$ at height $y$ is
$$
\ln \left(\frac{p}{p_{0}}\right)=\frac{M g}{R \alpha} \ln \left(\frac{T_{0}-\alpha y}{T_{0}}\right)
$$
where $p_{0}$ is the pressure at the earth's surface and $M$ is the molar mass for air. The coefficient $\alpha$ is called the lapse rate of temperature. It varies with atmospheric conditions, but an average value is about $0.6^{\circ} \mathrm{C} / 100 \mathrm{~m} .$ (b) Show that the above result reduces to the result of Example 18.4 (Section 18.1 ) in the limit that $\alpha \rightarrow 0$.
(c) With $\alpha=0.6^{\circ} \mathrm{C} / 100 \mathrm{~m},$ calculate $p$ for $y=8863 \mathrm{~m}$ and compare your answer to the result of Example 18.4. Take $T_{0}=288 \mathrm{~K}$ and $p_{0}=1.00 \mathrm{~atm}$

Christopher Dzorkpata
Christopher Dzorkpata
Numerade Educator
04:15

Problem 85

What is one reason the noble gases are preferable to air (which is mostly nitrogen and oxygen) as an insulating material?
(a) Noble gases are monatomic, so no rotational modes contribute to their molar heat capacity; (b) noble gases are monatomic, so they have lower molecular masses than do nitrogen and oxygen; (c) molecular radii in noble gases are much larger than those of gases that consist of diatomic molecules; (d) because noble gases are monatomic, they have many more degrees of freedom than do diatomic molecules, and their molar heat capacity is reduced by the number of degrees of freedom.

Shital Rijal
Shital Rijal
Numerade Educator
02:42

Problem 86

Estimate the ratio of the thermal conductivity of Xe to that of
He. (a) $0.015 ;$ (b) $0.061 ;$ (c) $0.10 ;$ (d) 0.17 .

Averell Hause
Averell Hause
Carnegie Mellon University
03:12

Problem 87

The rate of effusion - that is, leakage of a gas through tiny cracks-is proportional to $v_{\mathrm{rms}} .$ If tiny cracks exist in the material that's used to seal the space between two glass panes, how many times greater is the rate of He leakage out of the space between the panes than the rate of Xe leakage at the same temperature? (a) 370 times;
(b) 19 times; (c) 6 times; (d) no greater-the He leakage rate is the same as for Xe.

Shital Rijal
Shital Rijal
Numerade Educator