Consider four sealed, rigid containers with the following volumes: 50 mL, 100 mL, 250 mL, and 500 mL. If each of these contains

Question

erastova [34]

4 years ago

10

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?

Chemistry

1 answer:

dsp73 · Answer 1 · 2022-01-23T01:18:09+03:00

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.