In an isobaric process of an ideal gas, the ratio of work done by the system $(W)$ during the expansion and the heat exchanged $(Q)$ is $(\gamma = \frac{C_p}{C_v})$

$A$ gas expands under constant pressure $P$ from volume $V_1$ to $V_2$. The work done by the gas is

The equation of state for a gas is given by $PV = nRT + \alpha V$,where $n$ is the number of moles and $\alpha$ is a positive constant. The initial temperature and pressure of one mole of the gas contained in a cylinder are $T_0$ and $P_0$ respectively. The work done by the gas when its temperature doubles isobarically will be

In an isobaric expansion of an ideal gas,which of the following is zero?

If $\gamma$ is the ratio of molar specific heat at constant pressure to molar specific heat at constant volume for a gas,find the change in internal energy of $1 \, mol$ of the gas when its volume changes from $V$ to $2V$ at constant pressure $P$.

$A$ graph is drawn between absolute temperature and volume of $3$ moles of helium gas as shown in the figure. If $5 \text{ cal}$ of heat is used in the process, then the work done is (in $\text{ J}$)