An ideal monoatomic gas of $1.5$ moles is heated at a constant pressure of $2 \,atm$ so that its temperature increases from $30^{\circ} C$ to $130^{\circ} C$. The work done by the gas is (Universal gas constant $R = 8.3 \,J \,mol^{-1} \,K^{-1}$). (in $\,J$)

Two moles of helium gas are taken over the cycle $ABCDA$,as shown in the $P-T$ diagram. Assuming the gas to be ideal,the work done on the gas in taking it from $A$ to $B$ is ...... $R$.

$A$ 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

When an ideal gas $(\gamma = 5/3)$ is heated under constant pressure,what percentage of the given heat energy will be utilized in doing external work (in $\%$)?

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 ..... $cal$.

$10 \text{ mole}$ of an ideal gas is undergoing the process shown in the figure. The heat involved in the process from $P_1$ to $P_2$ at constant volume $V = 1 \text{ m}^3$ is $\alpha \text{ Joule}$ ($P_1 = 21.7 \text{ Pa}$, $P_2 = 30 \text{ Pa}$, $C_v = 21 \text{ J/K} \cdot \text{mol}$, $R = 8.3 \text{ J/mol} \cdot \text{K}$). The value of $\alpha$ is . . . . . . .