$A$ monoatomic gas is compressed adiabatically to $1/8$ of its initial volume. What happens to the gas pressure? $(\gamma = 5/3)$

$A$ sample of gas with $\gamma=1.5$ is taken through an adiabatic process in which the volume is compressed from $1200 \, cm^3$ to $300 \, cm^3$. If the initial pressure is $200 \, kPa$,find the absolute value of the work done by the gas in the process in Joules.

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

The adiabatic bulk modulus of a perfect gas at pressure $P$ is given by:

The initial pressure and volume of a given mass of an ideal gas (with $\frac{C_{p}}{C_{V}}=\gamma$),taken in a cylinder fitted with a piston,are $p_{0}$ and $V_{0}$ respectively. At this stage,the gas has the same temperature as that of the surrounding medium,which is $T_{0}$. It is adiabatically compressed to a volume equal to $\frac{V_{0}}{2}$. Subsequently,the gas is allowed to come to thermal equilibrium with the surroundings. What is the heat released to the surrounding?

$A$ monoatomic gas $\left(\gamma=\frac{5}{3}\right)$ at a pressure of $4 \text{ atm}$ is compressed adiabatically so that its temperature rises from $27^{\circ} \text{C}$ to $327^{\circ} \text{C}$. The pressure of the gas in its final state is