$A$ cyclic process of a thermodynamic system is taken through $a \to b \to c \to d \to a$ as shown in the $P-V$ diagram. The work done by the gas along the path $b \to c$ is

The temperature of $3.00 \, mol$ of an ideal diatomic gas is increased by $40.0^{\circ} C$ without changing the pressure of the gas. The molecules in the gas rotate but do not oscillate. If the ratio of change in internal energy of the gas to the amount of work done by the gas is $\frac{x}{10}$,then the value of $x$ (round off to the nearest integer) is ..... . (Given $R = 8.31 \, J \, mol^{-1} K^{-1}$)

$A$ monoatomic ideal gas is heated at constant pressure. The percentage of total heat used in changing the internal energy is (in $\%$)

$n$ 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

$A$ diatomic gas,having $C_{p} = \frac{7}{2} R$ and $C_{v} = \frac{5}{2} R$,is heated at constant pressure. The ratio $dU : dQ : dW$ is:

$A$ monoatomic gas is supplied heat $Q$ very slowly keeping the pressure constant. The work done by the gas will be