Answer:
A gas behaves more like an 'ideal' gas at a higher temperature and lower pressure.
Explanation:
do to intermolecular forces becomes less significant compared to kinetic energy and the size of the molecules become less significant to the empty space between them.
Gases are most likely to behave ideally at high temperature and low pressure.
Gases tend to operate ideally at low and high temperatures because potential energy is less important than kinetic energy due to intramolecular forces. Also, the size of the molecule is less important in relation to the free space between the molecules.
Gasworks very ideally at high temperatures and low pressures. High temperature means that the molecules move fast and do not stick together. Low pressure means that the molecules are farther apart and have less interaction.
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