Assertion (A): When an ideal gas is compresse | vedclass

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(A) In an adiabatic compression,work is done on the gas,which increases its internal energy. Since the internal energy of an ideal gas is directly pro

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$A$ and $R$ are true and $R$ is the correct explanation of $A$.

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(A) In an adiabatic compression,work is done on the gas,which increases its internal energy. Since the internal energy of an ideal gas is directly proportional to its absolute temperature $(U \propto T)$,the temperature of the gas increases.According to the kinetic theory of gases,the average kinetic energy of gas molecules is given by $K_{avg} = \frac{3}{2} k_B T$. As the temperature $T$ increases,the average kinetic energy also increases.This increase in kinetic energy occurs because,during compression,the molecules collide with the moving piston (wall). When a molecule hits a wall moving towards it,the molecule gains speed (and thus kinetic energy) due to the elastic collision,similar to a ball bouncing off a moving bat. Therefore,both the assertion and the reason are true,and the reason correctly explains the assertion.

Assertion $(A)$: When an ideal gas is compressed adiabatically,its temperature and the average kinetic energy of the gas molecules increase.
Reason $(R)$: The kinetic energy increases because of collisions of molecules with the moving parts of the wall.

Similar Questions

The $P-V$ diagram for two adiabatic processes is given. Curves $1$ and $2$ correspond to:

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Assertion $(A)$: When an ideal gas is compressed adiabatically,its temperature and the average kinetic energy of the gas molecules increase.Reason $(R)$: The kinetic energy increases because of collisions of molecules with the moving parts of the wall.