Which of the following graphs between pressure $(P)$ and volume $(V)$ correctly shows an isochoric process?

Calculate the work done when the volume of a gas increases by $0.25\,m^3$ at a constant pressure of $10^3\,N/m^2$.

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:

In an isochoric process,if ${T_1} = {27^o}C$ and ${T_2} = {127^o}C$,then ${P_1}/{P_2}$ will be equal to:

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 $(\gamma = \frac{C_p}{C_v})$

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