Consider four sealed, rigid containers with the following volumes: 50 mL, 100 mL, 250 mL, and 500 mL. If each of these contains. 25 moles of helium gas at standard temperature, which container would have the greatest pressure?

Question

Moshe Bradford

Chemistry

16 September, 18:48

Consider four sealed, rigid containers with the following volumes: 50 mL, 100 mL, 250 mL, and 500 mL. If each of these contains. 25 moles of helium gas at standard temperature, which container would have the greatest pressure?

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Answers (1)

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Jasmine Hammond · Answer 1

First, we assume that helium behaves as an ideal gas such that the ideal gas law is applicable.

PV = nRT

where P is pressure, V is volume, n is number of moles, R is universal gas constant, and T is temperature. From the equation, if n, R, and T are constant, there is an inverse relationship between P and V. From the given choices, the container with the greatest pressure would be the 50 mL.