$A$ 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:

One mole of an ideal gas $(\gamma = 1.4)$ is adiabatically compressed so that its temperature rises from $27\,^{\circ}C$ to $35\,^{\circ}C$. The change in the internal energy of the gas is .... $J$ (given $R = 8.3 \,J/mol/K$)

$A$ diesel engine has a compression ratio of $20:1$. If the initial pressure is $1 \times 10^5 \ Pa$ and the initial volume of the cylinder is $1 \times 10^{-3} \ m^3$, then how much work does the gas do during the compression (in $J$)? (Assume the process as adiabatic) $(C_V=20.8 \ J/mol \ K, \gamma=1.4, (20)^{1.4}=66.3)$

$5.6 \ L$ of Helium gas at $STP$ is compressed adiabatically to $0.7 \ L$. If the initial temperature is $T_1$,then the work done during the process is...?

An ideal gas at a pressure of $1 \text{ atm}$ and temperature of $27^{\circ}C$ is compressed adiabatically until its pressure becomes $8$ times the initial pressure. The final temperature is ..... $^{\circ}C$ (given $\gamma = 3/2$).

In an adiabatic expansion of an ideal gas,the product of pressure and volume: