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    Explain why the internal energy of a gas differs from that of its liquid phase? I've managed to get one mark for saying how the potential energy of a gas is higher, however the mark scheme isn't very clear on how to get the second mark. It just says to relate the temperature to the kinetic energy of the gas and liquid. Can anyone give me a model answer please?

    Depending on the course you're doing, you may or may not be expected to recall that the average KE is directly proportional to Kelvin temp via the equation

    average ke = 3/2 kT

    Also, if it's not an ideal gas. the potential energy will also be greater since the distance between the particiles is greater than in a liquid. This doesn't apply to an ideal gas because we assume that there are no forces of attraction between the particles.
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