In an $H_2$ gas process, $PV^2 = \text{constant}$. The ratio of work done by the gas to the change in its internal energy is:

During an experiment, an ideal gas is found to obey an additional law $VP^2 = \text{constant}$. The gas is initially at temperature $T$ and volume $V$. What will be the temperature of the gas when it expands to a volume $2V$?

The pressure and volume of an ideal gas are related as $PV^{3/2} = K$ (constant). The work done when the gas is taken from state $A(P_1, V_1, T_1)$ to state $B(P_2, V_2, T_2)$ is:

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:

$A$ diatomic gas undergoes a process represented by $PV^{1.3} = \text{constant}$. Choose the incorrect statement.

$1 \, \text{mole}$ of an ideal monoatomic gas at temperature $T_0$ expands slowly according to the law $P = KV$,where $K$ is a constant. If the final temperature of the gas is $2T_0$,find the heat supplied to the gas.