There are are two ways to make a gas hot. This is summed up quite neatly by the First Law of Thermodynamics:
ΔU = Q + Won
This law says that ΔU, the increase in internal energy of a system, can be brought about by
(1) Q, supplying heat to the system, or/and
(2) Won, doing work on the system.
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Macroscopically speaking, to do work on a gas is to compress it. Yup, work must be done against the gas pressure to force the gas into to a smaller volume.
Microscopically speaking, compressing a gas must involve a surface, let’s say a piston, charging into the gas. During this process, the piston is like a giant tennis racket smashing back all the trillions of tennis balls, i.e. the gas molecules, that happen to collide into it.
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These gas molecules were sent flying back at higher speed than before. Since the average KE of the gas molecules increases, and the temperature of the gas increases.