Which of the following best explains why the molar volume of a real gas becomes…
CHEMISTRY · Single correct · AP · Chemistry · Properties of Substances and Mixtures · Properties of Substances and Mixtures
Problem
Which of the following best explains why the molar volume of a real gas becomes greater than the value calculated using the ideal gas law when the gas is compressed to very high pressure at constant temperature?
(a) Intermolecular attractions become significant and reduce the effective pressure, so a larger volume is required to balance the external pressure.
(b) Compression raises the temperature of the gas, and the higher kinetic energy causes the gas to occupy a larger volume than predicted.
(c) The finite volume occupied by the gas particles becomes a significant fraction of the container volume, so the gas cannot be compressed as much as an ideal gas.
(d) Strong short-range repulsive forces between closely packed molecules raise the internal pressure, preventing further compression and leading to a larger molar volume.