During an adiabatic process, the pressure of a gas is proportional to the cube of its temperature. The value of $C_p / C_V$ for that gas is

The volume of air increases by $5\%$ in its adiabatic expansion. The percentage decrease in its pressure will be ...... $\%$

The pressure $P_{1}$ and density $d_{1}$ of a diatomic gas $\left(\gamma = \frac{7}{5}\right)$ change suddenly to $P_{2} (> P_{1})$ and $d_{2}$ respectively during an adiabatic process. The temperature of the gas increases and becomes $......$ times its initial temperature. (Given $\frac{d_{2}}{d_{1}} = 32$)

For adiabatic processes $\left( \gamma = \frac{C_p}{C_v} \right)$,which of the following relations is correct?

What is the change in temperature when work is done by a gas in an adiabatic process?

Initially,the pressure of $1 \text{ mole}$ of an ideal gas is $10^5 \text{ Nm}^{-2}$ and its volume is $16 \text{ litres}$. When it is adiabatically compressed,its final volume is $2 \text{ litres}$. Calculate the work done on the gas. [Given: Molar specific heat at constant volume $C_v = \frac{3R}{2}$] (in $\text{ kJ}$)