$A$ given system undergoes a change in which the work done by the system equals the decrease in its internal energy. The system must have undergone an

One mole of an ideal gas at an initial temperature of $T \ K$ does $6R \ J$ of work adiabatically. If the ratio of specific heats of this gas at constant pressure and at constant volume is $5/3$,the final temperature of the gas will be:

$A$ monatomic gas at a pressure of $100 \text{ kPa}$ expands adiabatically such that its final volume becomes $8$ times its initial volume. If the work done during the process is $180 \text{ J}$, then the initial volume of the gas is (in $\text{ cm}^3$)

During an adiabatic expansion of $2\, moles$ of a gas,the change in internal energy was found to be $-50\, J$. The work done during the process is ...... $J$.

Is it possible to increase the temperature of a gas without adding heat to it? Explain.

$A$ diatomic gas initially at $18^oC$ is compressed adiabatically to one-eighth of its original volume. The temperature after compression will be