(a) One assumption of the Ideal Gas Law is that the actual volume occupied by the molecules themselves is much less than the total volume, which includes the space between molecules. Consider 1 mole of helium (He) gas. (i) Estimate (in powers of 10) the volume occupied by 1 mole of He atoms, if the radius of one He atom is 31 pm [the "p" stands for pico, which represents one trillionth]. (ii) How does this value compare to the total volume occupied by 1 mole of He gas at standard temperature and pressure, 22.4 L? (Standard temperature and pressure refer to 0°C and 1 atm, respectively) (b) Suppose a planetary atmosphere consists of a strongly ionized gas. Would you expect the Ideal Gas Law to apply to this atmosphere? Why or why not?

(a) One assumption of the Ideal Gas Law is that the actual volume occupied by the molecules themselves is much less than the total volume, which includes the space between molecules. Consider 1 mole of helium (He) gas. (i) Estimate (in powers of 10) the volume occupied by 1 mole of He atoms, if the radius of one He atom is 31 pm [the "p" stands for pico, which represents one trillionth]. (ii) How does this value compare to the total volume occupied by 1 mole of He gas at standard temperature and pressure, 22.4 L? (Standard temperature and pressure refer to 0°C and 1 atm, respectively) (b) Suppose a planetary atmosphere consists of a strongly ionized gas. Would you expect the Ideal Gas Law to apply to this atmosphere? Why or why not?

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter3: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 92AP: Two moles of a monatomic ideal gas such as oxygen is compressed adiabatically and reversibly from a...

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