In a given process for an ideal gas,$dW = 0$ and $dQ < 0$. Then for the gas:

One mole of an ideal gas is contained within a cylinder by a frictionless piston and is initially at temperature $T$. The pressure of the gas is kept constant while it is heated and its volume doubles. If $R$ is the molar gas constant,the work done by the gas in increasing its volume is

In an isobaric process of an ideal gas,the ratio of heat supplied and work done by the system $\left(\frac{Q}{W}\right)$ is given by $\left[\frac{C_{P}}{C_{V}}=\gamma\right]$.

The temperature of $1$ mole of an ideal monoatomic gas is increased by $50^{\circ} C$ at constant pressure. The total heat added and change in internal energy are $E_1$ and $E_2$,respectively. If $\frac{E_1}{E_2}=\frac{x}{9}$,then the value of $x$ is . . . . . . .

The ratio of work done by an ideal rigid diatomic gas to the heat supplied to the gas in an isobaric process is (in $/7$)

Describe the nature of $P-V$ diagrams for isobaric and isochoric processes.