$600 \mathrm{J}$ of heat is added to a monoatomic gas in a process in which the gas performs a work of $150 \mathrm{J}$. The molar heat capacity for the process is

$p‐T$ diagram of one mole of an ideal monoatomic gas is shown. Processes $AB$ and $CD$ are adiabatic. Work done in the complete cycle is

The given figure shows the variation of force applied by ideal gas on a piston which undergoes a process during which piston position changes from $0.1$ to $0.4 \mathrm{m}$. If the internal energy of the system at the end of the process is $2.5 \mathrm{J}$ higher, then the heat absorbed during the process is

A thermodynamical process is shown in the figure with $p_{\mathrm{A}}=3\times p_{\mathrm{atm}}$, $V_{\mathrm{A}}=2\times {10}^{-4} {\mathrm{m}}^3$, $p_{\mathrm{B}}=8\times p_{\mathrm{atm}}$, $V_{\mathrm{C}}=5\times {10}^{-4} {\mathrm{m}}^3$
In the process $AB$ and $BC$, $600 \mathrm{J}$ and $200 \mathrm{J}$ heat are added to the system. Find the change in internal energy of the system in the process $CA$. $\left[1p_{\mathrm{atm}}={10}^5 \mathrm{N} {\mathrm{m}}^{-2}\right]$

A gas takes part in two processes, in which it is heated from the same initial state $1$ to the same final temperature. The processes are shown on the $p‐V$ diagram by the straight lines $1‐3$, $1‐2$ and $2‐3$ are the points on the same isothermal curve. $Q_1$ and $Q_2$ are the heat transfer along with the two processes. Then,