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 ..... $cal$.

At constant pressure,what fraction of the heat supplied to an ideal gas is converted into mechanical work?

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

An ideal gas undergoes the process $1 \rightarrow 2$ as shown in the figure. The heat supplied and work done in the process are $\Delta Q$ and $\Delta W$ respectively. The ratio $\Delta Q : \Delta W$ is

An ideal diatomic gas is heated at constant pressure. The ratio of the work done to the heat supplied is

The change in the internal energy of $3$ moles of a gas heated at constant volume from $20^{\circ}C$ to $40^{\circ}C$ is $1080 \ J$. The molar specific heat of the gas at constant volume in $J \ mol^{-1} \ K^{-1}$ is: