A gas is compressed adiabatically. Which one | vedclass

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(D) For an adiabatic process,the heat exchange $\Delta Q = 0$.According to the first law of thermodynamics,$\Delta Q = \Delta U + \Delta W$,where $\De

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There is no change in the internal energy.

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(D) For an adiabatic process,the heat exchange $\Delta Q = 0$.According to the first law of thermodynamics,$\Delta Q = \Delta U + \Delta W$,where $\Delta U$ is the change in internal energy and $\Delta W$ is the work done by the gas.Since $\Delta Q = 0$,we have $\Delta U = -\Delta W$.In adiabatic compression,the volume decreases $(V \downarrow)$,so the work done by the gas $\Delta W$ is negative $(-ve)$.Therefore,$\Delta U = -(-ve) = +ve$,which means the internal energy increases.Since internal energy is a function of temperature,an increase in internal energy implies an increase in temperature $(T \uparrow)$.Thus,the statement 'There is no change in the internal energy' is $NOT$ true.

$A$ gas is compressed adiabatically. Which one of the following statements is $NOT$ true?

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