$A$ diatomic gas $\left(C_P = \frac{7}{2} R\right)$ does $200 \ J$ of work when it is expanded isobarically. The heat given to the gas in the process is (in $J$)

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

$A$ graph is drawn between absolute temperature and volume of $3$ moles of helium gas as shown in the figure. If $5 \text{ cal}$ of heat is used in the process, then the work done is (in $\text{ J}$)

The work done by a gas is maximum when it expands from a volume $V_1$ to $V_2$. This expansion is:

$n$ moles of an ideal gas with constant volume heat capacity $C_v$ undergo an isobaric expansion by a certain volume. The ratio of the work done in the process to the heat supplied is

How much work is to be done in decreasing the volume of an ideal gas by an amount of $2.4 \times 10^{-4} \ m^3$ at normal temperature and constant normal pressure of $1 \times 10^5 \ N/m^2$ (in $J$)?