$A$ polyatomic gas $(\gamma = 4/3)$ is compressed to $(1/8)^{\text{th}}$ of its initial volume adiabatically. If its initial pressure is $P_0$,what will be its new pressure (in $P_0$)?

The adiabatic modulus of elasticity of a gas is $2.1 \times 10^5 \ N/m^2$. What will be its isothermal modulus of elasticity? (Given: $\frac{C_p}{C_v} = 1.4$)

The $P-V$ diagram for two gases during an adiabatic process is shown in the figure. Curves $A$ and $B$ correspond to:

$A$ gas for which $\gamma = 1.5$ is suddenly compressed to $\frac{1}{4}$ of its initial volume. What is the ratio of the final pressure to the initial pressure?

Under an adiabatic process,the volume of an ideal gas gets doubled. Consequently,the mean collision time between the gas molecules changes from $\tau_{1}$ to $\tau_{2}$. If $\frac{C_{p}}{C_{v}}=\gamma$ for this gas,then a good estimate for $\frac{\tau_{2}}{\tau_{1}}$ is given by:

Initial pressure and volume of a monoatomic ideal gas are $P$ and $V$. The change in internal energy of this gas in adiabatic expansion to volume $V_{final} = 27V$ is . . . . . . $J$.