$A$ diatomic ideal gas undergoes a thermodynamic change according to the $P-V$ diagram shown in the figure. The heat given to the gas in process $AB$ is: (in $, P_0 V_0$)

$A$ diatomic gas $(\gamma = 1.4)$ does $100 \ J$ of work when it is expanded isobarically. Then the heat given to the gas is . . . . . . $J$.

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

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

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

In an isochoric process,if $t_1 = 27^{\circ}C$ and $t_2 = 127^{\circ}C$,then $\frac{P_1}{P_2}$ will be equal to [$P_1$ and $P_2$ are the pressures at $t_1^{\circ}C$ and $t_2^{\circ}C$ respectively].