The $P-V$ diagram for an ideal gas in a piston-cylinder assembly undergoing a thermodynamic process is shown in the figure. The process is

The work done by $6$ moles of helium gas when its temperature increases by $20^{\circ} C$ at constant pressure is (Universal gas constant $R = 8.31 \ J \ mol^{-1} \ K^{-1}$) (in $J$)

Two containers $A$ and $B$ with pistons contain a diatomic gas at $300\, K$. The piston in container $A$ is free to move,while the piston in container $B$ is fixed. Both containers are supplied with the same amount of heat. If the temperature in container $A$ increases by $30\, K$,by how many $K$ will the temperature in container $B$ increase? Both containers contain the same gas.

Work done by $0.1$ mole of a gas at $27^{\circ}C$ to double its volume at constant pressure is ....... $cal$ $(R = 2 \, cal \, mol^{-1} \, K^{-1})$.

$A$ monoatomic gas is supplied heat $Q$ very slowly keeping the pressure constant. The work done by the gas will be

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