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    A question about the first law of thermodynamics states:

    ∂U = ∂Q + ∂W (U= internal enegy, Q=thermal energy supplied to system, W=work done on system)

    An ideal gas is compressed at constant temperature, what is the effect on U, q and W?


    The answer is that U remains constant, q decreases and W increases.

    What I want to know is if a gas is compressed why does q decrease?
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    I think it's because at a constant temperature, when the gas is compressed less movement is possible. Therefore as temperature is related to kinetic energy and movement of particles, the thermal energy must decrease as there is less movement.
 
 
 
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