$A$ gas obeys $P^2V = \text{constant}$. The initial temperature and volume are $T_0$ and $V_0$. If the gas expands to a volume of $2V_0$,the final temperature is:

$A$ diatomic gas follows the equation $PV^m =$ constant during a process. What should be the value of $m$ such that its molar heat capacity during the process is equal to $R$?

An ideal gas follows a process described by the equation $PV^2 = C$ from the initial $(P_1, V_1, T_1)$ to final $(P_2, V_2, T_2)$ thermodynamic states,where $C$ is a constant. Then:

$A$ monoatomic gas is taken through a process $TP^{-1/3} = \text{constant}$. If heat is given to the gas, what happens to its temperature?

During an experiment, an ideal gas obeys an additional equation of state $P^2V = \text{constant}$. The initial temperature and volume of the gas are $T$ and $V$ respectively. When it expands to volume $2V$, its temperature will be:

An ideal gas expands in such a way that $PV^2 = \text{constant}$ throughout the process.