During an adiabatic process,the volume of a gas is found to be inversely proportional to the cube of its temperature. The ratio of $\frac{C_p}{C_v}$ for the gas is

$A$ gas having $\gamma = 5/2$ and volume $360 \text{ c.c.}$ is suddenly compressed to $90 \text{ c.c.}$ If the initial pressure of the gas is $P$,then the final pressure will be:

This question has Statement $1$ and Statement $2.$ Of the four choices given after the Statements,choose the one that best describes the two Statements.
Statement $1:$ In an adiabatic process,the change in internal energy of a gas is equal to the work done on/by the gas in the process.
Statement $2:$ The temperature of a gas remains constant in an adiabatic process.

$A$ monoatomic gas $\left( \gamma = \frac{5}{3} \right)$ is suddenly compressed to $\frac{1}{8}$ of its original volume. What will be the final pressure of the gas in terms of its initial pressure?

$A$ gas at normal temperature is suddenly compressed to one-fourth of its original volume. If $\frac{C_{p}}{C_{v}}=\gamma=1.5$,then the increase in its temperature is (in $K$)

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: $\frac{C_p}{C_v} = 1.4$)