$A$ 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 $\text{ J}$)

$A$ diatomic gas $(\gamma = 1.4)$ does $300 \ J$ of work when expanded isobarically. The heat given to the gas in this process is: (in $J$)

Which one of the following equations specifies an isochoric process?
$[Q = \text{heat supplied, } \Delta p = \text{change in pressure, } \Delta V = \text{change in volume, } \Delta T = \text{change in temperature}]$

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 $\%$)?

$10 \text{ mole}$ 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 . . . . . . .

In thermodynamics,for an isochoric process,which one of the following statements is $INCORRECT$?