In an isobaric process of an ideal gas,the ratio of work done by the system to the heat supplied $\left(\frac{W}{Q}\right)$ 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

$A$ sample of gas expands from volume ${V_1}$ to ${V_2}$. The amount of work done by the gas is greatest when the expansion is

An ideal monoatomic gas of $1.5$ moles is heated at a constant pressure of $2 \,atm$ so that its temperature increases from $30^{\circ} C$ to $130^{\circ} C$. The work done by the gas is (Universal gas constant $R = 8.3 \,J \,mol^{-1} \,K^{-1}$). (in $\,J$)

The work done to double the volume of $0.1 \ mol$ of a gas at constant pressure and a temperature of $27 \ ^\circ C$ is equal to ..... $cal$.

$A$ monoatomic ideal gas expands at constant pressure,with heat $Q$ supplied. The fraction of $Q$ which goes as work done by the gas is