# Problems & Exercises

### 13.1 Temperature

What is the Fahrenheit temperature of a person with a $\text{39}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ fever?

Frost damage to most plants occurs at temperatures of $\text{28}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{F}$ or lower. What is this temperature on the Kelvin scale?

To conserve energy, room temperatures are kept at $\text{68}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{F}$ in the winter and $\text{78}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{F}$ in the summer. What are these temperatures on the Celsius scale?

A tungsten light bulb filament may operate at 2,900 K. What is its Fahrenheit temperature? What is this on the Celsius scale?

The surface temperature of the Sun is about 5,750 K. What is this temperature on the Fahrenheit scale?

One of the hottest temperatures ever recorded on the surface of Earth was $\text{134}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{F}$ in Death Valley, CA. What is this temperature in Celsius degrees? What is this temperature in Kelvin?

(a) Suppose a cold front blows into your locale and drops the temperature by 40 Fahrenheit degrees. How many degrees Celsius does the temperature decrease when there is a $\text{40}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{F}$ decrease in temperature? (b) Show that any change in temperature in Fahrenheit degrees is nine-fifths the change in Celsius degrees.

(a) At what temperature do the Fahrenheit and Celsius scales have the same numerical value? (b) At what temperature do the Fahrenheit and Kelvin scales have the same numerical value?

### 13.2 Thermal Expansion of Solids and Liquids

The height of the Washington Monument is measured to be 170 m on a day when the temperature is $\text{35}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$. What will its height be on a day when the temperature falls to $\u2013\text{10}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? Although the monument is made of limestone, assume that its thermal coefficient of expansion is the same as marble’s.

How much taller does the Eiffel Tower become at the end of a day when the temperature has increased by $\text{15}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? Its original height is 321 m and you can assume it is made of steel.

What is the change in length of a 3-cm-long column of mercury if its temperature changes from $\text{37}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ to $\text{40}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}\text{,}$ assuming the mercury is unconstrained?

How large an expansion gap should be left between steel railroad rails if they may reach a maximum temperature $\text{35}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ greater than when they were laid? Their original length is 10 m.

You are looking to purchase a small piece of land in Hong Kong. The price is *only* $60,000 per square meter! The land title says the dimensions are $\text{20}\phantom{\rule{0.25em}{0ex}}\text{m}\phantom{\rule{0.20em}{0ex}}\times \phantom{\rule{0.20em}{0ex}}\text{30 m}\text{.}$ By how much would the total price change if you measured the parcel with a steel tape measure on a day when the temperature was $\text{20}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ above normal?

Global warming will produce rising sea levels partly due to melting ice caps but also due to the expansion of water as average ocean temperatures rise. To get some idea of the size of this effect, calculate the change in length of a column of water 1 km high for a temperature increase of $1\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}\text{.}$ Note that this calculation is only approximate because ocean warming is not uniform with depth.

Show that 60 L of gasoline originally at $\text{15}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ will expand to 61.1 L when it warms to $\text{35}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C,}$ as claimed in Example 13.4.

(a) Suppose a meter stick made of steel and one made of invar—an alloy of iron and nickel—are the same length at $0\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$. What is their difference in length at $\text{22}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? (b) Repeat the calculation for two 30-m-long surveyor’s tapes.

(a) If a 500-mL glass beaker is filled to the brim with ethyl alcohol at a temperature of $5\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C,}$ how much will overflow when its temperature reaches $\text{22}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? (b) How much less water would overflow under the same conditions?

Most automobiles have a coolant reservoir to catch radiator fluid that may overflow when the engine is hot. A radiator is made of copper and is filled to its 16.0-L capacity when at $\text{10\xbaC}\text{.}$ What volume of radiator fluid will overflow when the radiator and fluid reach their $\text{95\xbaC}$ operating temperature, given that the fluid’s volume coefficient of expansion is $\beta =\text{400}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{\u20136}/\text{\xba}\text{C}$? Note that this coefficient is approximate, because most car radiators have operating temperatures of greater than $\text{95}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}\text{.}$

A physicist makes a cup of instant coffee and notices that, as the coffee cools, its level drops 3 mm in the glass cup. Show that this decrease cannot be due to thermal contraction by calculating the decrease in level if the $\text{350}\phantom{\rule{0.25em}{0ex}}{\text{cm}}^{3}$ of coffee is in a 7-cm-diameter cup and decreases in temperature from $\text{95}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}\phantom{\rule{0.25em}{0ex}}$to$\phantom{\rule{0.25em}{0ex}}\text{45}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}\text{.}$ Most of the drop in level is actually due to escaping bubbles of air.

(a) The density of water at $0\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ is very nearly $\text{1,000}\phantom{\rule{0.25em}{0ex}}{\text{kg/m}}^{3}$ it is actually $9\text{99}\text{.}{\text{84 kg/m}}^{3}$, whereas the density of ice at $0\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ is $9{\text{17 kg/m}}^{3}$. Calculate the pressure necessary to keep ice from expanding when it freezes, neglecting the effect such a large pressure would have on the freezing temperature. This problem gives you only an indication of how large the forces associated with freezing water might be. (b) What are the implications of this result for biological cells that are frozen?

Show that $\beta \approx \mathrm{3\alpha},$ by calculating the change in volume $\text{\Delta}V$ of a cube with sides of length $L\text{.}$

### 13.3 The Ideal Gas Law

Under what circumstances would you expect a gas to behave significantly differently than predicted by the ideal gas law? How would these differences in behavior be evident in plots of volume versus temperature—with pressure held fixed—and pressure versus volume—with temperature held fixed?

The gauge pressure in your car tires is $2\text{.}\text{50}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{5}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$ at a temperature of $\text{35}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ when you drive it onto a ferry boat to Alaska. What is their gauge pressure later, when their temperature has dropped to $\u2013\text{40}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$?

Convert an absolute pressure of $7\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{5}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$ to gauge pressure in ${\text{lb./in.}}^{2}\text{.}$ This value was stated to be just less than ${\text{90lb/in}}^{\text{2}}$ in Example 13.9. Is it?

Suppose a gas-filled incandescent light bulb is manufactured so that the gas inside the bulb is at atmospheric pressure when the bulb has a temperature of $\text{20}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$. (a) Find the gauge pressure inside such a bulb when it is hot, assuming its average temperature is $\text{60}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ an approximation—and neglecting any change in volume due to thermal expansion or gas leaks. (b) The actual final pressure for the light bulb will be less than calculated in part (a) because the glass bulb will expand. What will the actual final pressure be, taking this into account? Is this a negligible difference?

Large helium-filled balloons are used to lift scientific equipment to high altitudes. (a) What is the pressure inside such a balloon if it starts out at sea level with a temperature of $\text{10}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ and rises to an altitude where its volume is twenty times the original volume and its temperature is $\u2013\text{50}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? (b) What is the gauge pressure? Assume atmospheric pressure is constant.

Confirm that the units of $\text{nRT}$ are those of energy for each value of $R$: (a) $8\text{.}\text{31}\phantom{\rule{0.25em}{0ex}}\text{J/mol}\cdot \text{K}$, (b) $1\text{.}\text{99 cal/mol}\cdot \text{K}$, and (c) $0\text{.}\text{0821 L}\cdot \text{atm/mol}\cdot \text{K}$.

In the text, it was shown that $N/V=2\text{.}\text{68}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{\text{25}}\phantom{\rule{0.25em}{0ex}}{\text{m}}^{-3}$ for gas at STP. (a) Show that this quantity is equivalent to $N/V=2\text{.}\text{68}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{\text{19}}\phantom{\rule{0.25em}{0ex}}{\text{cm}}^{-3},$ as stated. (b) About how many atoms are there in one ${\text{\mu m}}^{3}$ (a cubic micrometer) at STP? (c) What does your answer to part (b) imply about the separation of atoms and molecules?

Calculate the number of moles in the 2-L volume of air in the lungs of the average person. Note that the air is at $\text{37\xbaC}$ (body temperature).

An airplane passenger has $\text{100}\phantom{\rule{0.25em}{0ex}}{\text{cm}}^{3}$ of air in his stomach just before the plane takes off from a sea-level airport. What volume will the air have at cruising altitude if cabin pressure drops to $7\text{.}\text{50}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{4}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}?$

Suppose the data in the following table was taken at constant temperature. Plot the data, with the pressure on the vertical axis and the volume on the horizontal axis. Use the last data point to determine what the relationship between *P* and *V* would be if the gas were ideal. Then plot the corresponding curve on the graph and identify where deviations from the ideal gas law first become evident. Why does the last data point most likely represent ideal gas behavior? Why do deviations from ideal gas behavior occur?

V (m^{3}) |
P (10^{5} Pa) |
---|---|

0.001 | 30.9 |

0.002 | 16.5 |

0.003 | 10.8 |

0.004 | 7.73 |

0.005 | 5.59 |

0.006 | 4.36 |

0.007 | 3.56 |

0.008 | 3.12 |

0.009 | 2.77 |

0.010 | 2.49 |

(a) What is the volume (in ${\text{km}}^{3}$) of Avogadro’s number of sand grains if each grain is a cube and has sides that are 1.0 mm long? (b) How many kilometers of beaches in length would this cover if the beach averages 100 m in width and 10.0 m in depth? Neglect air spaces between grains.

An expensive vacuum system can achieve a pressure as low as $1\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{\u20137}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$ at $\text{20}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$. How many atoms are there in a cubic centimeter at this pressure and temperature?

The number density of gas atoms at a certain location in the space above our planet is about $1\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{\text{11}}\phantom{\rule{0.25em}{0ex}}{\text{m}}^{-3},$ and the pressure is $2\text{.}\text{75}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{\u2013\text{10}}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$ in this space. What is the temperature there?

A bicycle tire has a pressure of $7\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{5}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$ at a temperature of $\text{18}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ and contains 2 L of gas. What will its pressure be if you let out an amount of air that has a volume of $\text{100}\phantom{\rule{0.25em}{0ex}}{\text{cm}}^{3}$ at atmospheric pressure? Assume tire temperature and volume remain constant.

A high-pressure gas cylinder contains 50.0 L of toxic gas at a pressure of $1\text{.}\text{40}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{7}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$ and a temperature of $\text{25}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$. Its valve leaks after the cylinder is dropped. The cylinder is cooled to dry ice temperature $(\u2013\text{78}\text{.}5\phantom{\rule{0.25em}{0ex}}\text{\xba}\phantom{\rule{0.25em}{0ex}}\text{C})$ to reduce the leak rate and pressure so that it can be safely repaired. (a) What is the final pressure in the tank, assuming a negligible amount of gas leaks while being cooled and that there is no phase change? (b) What is the final pressure if one-tenth of the gas escapes? (c) To what temperature must the tank be cooled to reduce the pressure to 1 atm—assuming the gas does not change phase and that there is no leakage during cooling? (d) Does cooling the tank appear to be a practical solution?

Find the number of moles in 2 L of gas at $\text{35}\phantom{\rule{0.25em}{0ex}}\text{\xba}\phantom{\rule{0.25em}{0ex}}\text{C}$ and under $7\text{.}\text{41}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{7}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$ of pressure.

Calculate the depth to which Avogadro’s number of table tennis balls would cover Earth. Each ball has a diameter of 3.75 cm. Assume the space between balls adds an extra 25 percent to their volume and assume they are not crushed by their own weight.

(a) What is the gauge pressure in a $\text{25}\phantom{\rule{0.25em}{0ex}}\text{\xba}\phantom{\rule{0.25em}{0ex}}\text{C}$ car tire containing 3.60 mol of gas in a 30 L volume? (b) What will its gauge pressure be if you add 1 L of gas originally at atmospheric pressure and $\text{25}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? Assume the temperature returns to $\text{25}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ and the volume remains constant.

(a) In the deep space between galaxies, the density of atoms is as low as ${\text{10}}^{6}\phantom{\rule{0.25em}{0ex}}{\text{atoms/m}}^{3},$ and the temperature is a frigid 2.7 K. What is the pressure? (b) What volume (in ${\text{m}}^{3}$) is occupied by 1 mol of gas? (c) If this volume is a cube, what is the length of its sides in kilometers?

### 13.4 Kinetic Theory: Atomic and Molecular Explanation of Pressure and Temperature

Some incandescent light bulbs are filled with argon gas. What is ${v}_{\text{rms}}$ for argon atoms near the filament, assuming their temperature is 2,500 K?

Average atomic and molecular speeds $({v}_{\text{rms}})$ are large, even at low temperatures. What is ${v}_{\text{rms}}$ for helium atoms at 5 K, just one degree above helium’s liquefaction temperature?

(a) What is the average kinetic energy in joules of hydrogen atoms on the $\text{5,500}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ surface of the Sun? (b) What is the average kinetic energy of helium atoms in a region of the solar corona where the temperature is $6\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{5}\phantom{\rule{0.25em}{0ex}}\text{K}$?

The escape velocity of any object from Earth is 11.2 km/s. (a) Express this speed in m/s and km/h. (b) At what temperature would oxygen molecules (molecular mass is equal to 32 g/mol) have an average velocity ${v}_{\text{rms}}$ equal to Earth’s escape velocity of 11.1 km/s?

The escape velocity from the Moon is much smaller than from Earth and is only 2.38 km/s. At what temperature would hydrogen moleculesmolecular mass is equal to 2.016 g/molhave an average velocity ${v}_{\text{rms}}$ equal to the Moon’s escape velocity?

Nuclear fusion, the energy source of the Sun, hydrogen bombs, and fusion reactors, occurs much more readily when the average kinetic energy of the atoms is high—that is, at high temperatures. Suppose you want the atoms in your fusion experiment to have average kinetic energies of $6\text{.}\text{40}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{\u2013\text{14}}\phantom{\rule{0.25em}{0ex}}\text{J}$. What temperature is needed?

Suppose that the average velocity $({v}_{\text{rms}})$ of carbon dioxide moleculesmolecular mass is equal to 44 g/molin a flame is found to be $1\text{.}\text{05}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{5}\phantom{\rule{0.25em}{0ex}}\text{m/s}$. What temperature does this represent?

Hydrogen moleculesmolecular mass is equal to 2.016 g/molhave an average velocity ${v}_{\text{rms}}$ equal to 193 m/s. What is the temperature?

Much of the gas near the Sun is atomic hydrogen. Its temperature would have to be $1\text{.}5\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{7}\phantom{\rule{0.25em}{0ex}}\text{K}$ for the average velocity ${v}_{\text{rms}}$ to equal the escape velocity from the Sun. What is that velocity?

There are two important isotopes of uranium—${}^{\text{235}}\text{U}$ and ${}^{\text{238}}\text{U}$these isotopes are nearly identical chemically but have different atomic masses. Only ${}^{\text{235}}\text{U}$ is very useful in nuclear reactors. One of the techniques for separating themgas diffusionis based on the different average velocities ${v}_{\text{rms}}$ of uranium hexafluoride gas, ${\text{UF}}_{6}$. (a) The molecular masses for ${}^{\text{235}}\text{U}\phantom{\rule{0.25em}{0ex}}$${\text{UF}}_{6}$ and ${}^{\text{238}}\text{U}$$\phantom{\rule{0.25em}{0ex}}{\text{UF}}_{6}$ are 349 g/mol and 352 g/mol, respectively. What is the ratio of their average velocities? (b) At what temperature would their average velocities differ by 1 m/s? (c) Do your answers in this problem imply that this technique may be difficult?

### 13.6 Humidity, Evaporation, and Boiling

Dry air is 78.1 percent nitrogen. What is the partial pressure of nitrogen when the atmospheric pressure is $1\text{.}\text{01}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{5}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$?

(a) What is the vapor pressure of water at $\text{20}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? (b) What percentage of atmospheric pressure does this correspond to? (c) What percent of $\text{20}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ air is water vapor if it has 100 percent relative humidity? The density of dry air at $\text{20}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ is $1\text{.}\text{20}\phantom{\rule{0.25em}{0ex}}{\text{kg/m}}^{3}$.

Pressure cookers increase cooking speed by raising the boiling temperature of water above its value at atmospheric pressure. (a) What pressure is necessary to raise the boiling point to $\text{120}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? (b) What gauge pressure does this correspond to?

(a) At what temperature does water boil at an altitude of 1,500 mabout 5,000 ft.on a day when atmospheric pressure is $8\text{.}\text{59}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{4}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}\text{?}$ (b) What about at an altitude of 3,000 m (about 10,000 ft) when atmospheric pressure is $7\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{4}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}\text{?}$

What is the atmospheric pressure on top of Mt. Everest on a day when water boils there at a temperature of $\text{70}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C?}$

At a spot in the high Andes, water boils at $\text{80}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$, greatly reducing the cooking speed of potatoes, for example. What is atmospheric pressure at this location?

What is the relative humidity on a $\text{25}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ day when the air contains $\text{18}\phantom{\rule{0.25em}{0ex}}{\text{g/m}}^{3}$ of water vapor?

What is the density of water vapor in ${\text{g/m}}^{3}$ on a hot dry day in the desert when the temperature is $\text{40}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ and the relative humidity is 6.00 percent?

A deep-sea diver should breathe a gas mixture that has the same oxygen partial pressure as at sea level, where dry air contains 20.9 percent oxygen and has a total pressure of $1\text{.}\text{01}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{5}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$. (a) What is the partial pressure of oxygen at sea level? (b) If the diver breathes a gas mixture at a pressure of $2\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{6}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$, what percent oxygen should it be to have the same oxygen partial pressure as at sea level?

The vapor pressure of water at $\text{40}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ is $7\text{.}\text{34}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{3}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$. Using the ideal gas law, calculate the density of water vapor in ${\text{g/m}}^{3}$ that creates a partial pressure equal to this vapor pressure. The result should be the same as the saturation vapor density at that temperature $(\text{51}\text{.}{\text{1 g/m}}^{3})\text{.}$

Air in human lungs has a temperature of $\text{37}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ and a saturation vapor density of ${\text{44g/m}}^{\text{3}}$ (a) If 2 L of air is exhaled and very dry air inhaled, what is the maximum loss of water vapor by the person? (b) Calculate the partial pressure of water vapor having this density, and compare it with the vapor pressure of $6\text{.}\text{31}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{3}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$.

If the relative humidity is 90.0 percent on a muggy summer morning when the temperature is $\text{20}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$, what will it be later in the day when the temperature is $\text{30}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$, assuming the water vapor density remains constant?

Late on an autumn day, the relative humidity is 45 percent and the temperature is $\text{20}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$. What will the relative humidity be that evening when the temperature has dropped to $\text{10}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$, assuming constant water vapor density?

Atmospheric pressure atop Mt. Everest is $3\text{.}\text{30}\times {\text{10}}^{4}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$. (a) What is the partial pressure of oxygen there if it is 20.9 percent of the air? (b) What percent oxygen should a mountain climber breathe so that its partial pressure is the same as at sea level, where atmospheric pressure is $1\text{.}\text{01}\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{5}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}\text{?}$ (c) One of the most severe problems for those climbing very high mountains is the extreme drying of breathing passages. Why does this drying occur?

What is the dew pointthe temperature at which 100 percent relative humidity would occuron a day when relative humidity is 39 percent at a temperature of $\text{20}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$?

On a certain day, the temperature is $\text{25}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ and the relative humidity is 90 percent. How many grams of water must condense out of each cubic meter of air if the temperature falls to $\text{15}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? Such a drop in temperature can, thus, produce heavy dew or fog.

**Integrated Concepts**

The boiling point of water increases with depth, because pressure increases with depth. At what depth will fresh water have a boiling point of $\text{150}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$, if the surface of the water is at sea level?

**Integrated Concepts**

(a) At what depth in fresh water is the critical pressure of water reached, given that the surface is at sea level? (b) At what temperature will this water boil? (c) Is a significantly higher temperature needed to boil water at a greater depth?

**Integrated Concepts**

To get an idea of the small effect that temperature has on Archimedes’ principle, calculate the fraction of a copper block’s weight that is supported by the buoyant force in $0\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ water and compare this fraction with the fraction supported in $\text{95}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ water.

**Integrated Concepts**

If you want to cook in water at $\text{150}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$, you need a pressure cooker that can withstand the necessary pressure. (a) What pressure is required for the boiling point of water to be this high? (b) If the lid of the pressure cooker is a disk 25 cm in diameter, what force must it be able to withstand at this pressure?

**Unreasonable Results**

(a) How many moles per cubic meter of an ideal gas are there at a pressure of $1\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{\text{14}}\phantom{\rule{0.25em}{0ex}}{\text{N/m}}^{2}$ and at $0\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$? (b) What is unreasonable about this result? (c) Which premise or assumption is responsible?

**Unreasonable Results**

(a) An automobile mechanic claims that an aluminum rod fits loosely into its hole on an aluminum engine block because the engine is hot and the rod is cold. If the hole is 10 percent bigger in diameter than the $\text{22}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ rod, at what temperature will the rod be the same size as the hole? (b) What is unreasonable about this temperature? (c) Which premise is responsible?

**Unreasonable Results**

The temperature inside a supernova explosion is said to be $2\phantom{\rule{0.25em}{0ex}}\times \phantom{\rule{0.25em}{0ex}}{\text{10}}^{\text{13}}\phantom{\rule{0.25em}{0ex}}\text{K}$. (a) What would the average velocity ${v}_{\text{rms}}$ of hydrogen atoms be? (b) What is unreasonable about this velocity? (c) Which premise or assumption is responsible?

**Unreasonable Results**

Suppose the relative humidity is 80 percent on a day when the temperature is $\text{30}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$. (a) What will the relative humidity be if the air cools to $\text{25}\phantom{\rule{0.25em}{0ex}}\text{\xba}\text{C}$ and the vapor density remains constant? (b) What is unreasonable about this result? (c) Which premise is responsible?