The $P-V$ diagram of a diatomic ideal gas system undergoing a cyclic process is shown in the figure. The work done during the adiabatic process $CD$ is (use $\gamma=1.4$) (in $J$):

$A$ monoatomic gas $(\gamma = 5/3)$ initially at $27^{\circ} C$ having volume $V$ is suddenly compressed to one-eighth of its original volume $(V/8)$. What is the final temperature after the compression (in $K$)?

$\Delta U + \Delta W = 0$ is valid for

In adiabatic compression, the decrease in volume is associated with

$A$ vessel contains $0.15 \ \text{m}^3$ of a gas at pressure $8 \ \text{bar}$ and temperature $140^\circ \text{C}$ with $c_p = 3R$ and $c_v = 2R$. It is expanded adiabatically until the pressure falls to $1 \ \text{bar}$. The work done during this process is . . . . . . $\text{kJ}$.

The volume of an ideal gas $(\gamma=1.5)$ is changed adiabatically from $5 \ L$ to $4 \ L$. The ratio of initial pressure to final pressure is: