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

Pressure as molecular collisions with the walls, temperature as average kinetic energy, and the spread of molecular speeds in a gas.

College Physics 2e, 13.4 Kinetic Theory: Atomic and Molecular Explanation of Pressure and Temperature

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8 exercises

13.4 Exercise 1

If you consider a very small object such as a grain of pollen, in a gas, then the number of atoms and molecules striking its surface would also be relatively small. Would the grain of pollen experience any fluctuations in pressure due to statistical fluctuations in the number of gas atoms and molecules striking it in a given amount of time?

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13.4 Exercise 2

Two samples of ideal gas in separate containers have the same number of molecules and the same temperature, but the molecular mass of gas X is greater than that of gas Y. Which of the following correctly compares the average speed of the molecules of the gases and the average force the gases exert on their respective containers?

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13.4 Exercise 6

What is the average kinetic energy of a nitrogen molecule (N₂) if its rms speed is 560 m/s? At what temperature is this rms speed achieved?

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13.4 Exercise 9

Some incandescent light bulbs are filled with argon gas. What is $v_{\text{rms}}$ for argon atoms near the filament, assuming their temperature is 2500 K?

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13.4 Exercise 11

(a) What is the average kinetic energy in joules of hydrogen atoms on the $\text{5500} º \text{C}$ 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 $6 . \text{00} \times \text{10}^{5} \text{K}$ ?

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13.4 Exercise 13

The escape velocity from the Moon is much smaller than from Earth and is only 2.38 km/s. At what temperature would hydrogen molecules (molecular mass is equal to 2.016 g/mol) have an average velocity $v_{\text{rms}}$ equal to the Moon’s escape velocity?

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13.4 Exercise 15

Suppose that the average velocity $\left(v_{\text{rms}}\right)$ of carbon dioxide molecules (molecular mass is equal to 44.0 g/mol) in a flame is found to be $1 . \text{05} \times \text{10}^{5} \text{m}/\text{s}$ . What temperature does this represent?

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13.4 Exercise 17

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

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