In a cyclic process $A \rightarrow B \rightarrow C \rightarrow A$,the heat given to the gas is $5 \ J$. The work done during the process $C \rightarrow A$ is ............ $J$.

The figure given below shows the variation in the internal energy $U$ with volume $V$ of $2.0 \text{ mole}$ of an ideal gas in a cyclic process $abcda$. The temperatures of the gas during the processes $ab$ and $cd$ are $500 \text{ K}$ and $300 \text{ K}$ respectively. The heat absorbed by the gas during the complete process is .... $J$. (Take $R = 8.3 \text{ J/mol-K}$ and $\ln 2 = 0.69$)

Six moles of an ideal gas perform the cycle shown in the figure. If the temperatures are $T_A = 600 \, K$, $T_B = 800 \, K$, $T_C = 2200 \, K$, and $T_D = 1200 \, K$, the work done per cycle is ........ $kJ$.

$A$ thermodynamic system is taken through the cycle $PQRSP$ process as shown in the figure. The net work done by the system is .... $J$. (Note: $1 \text{ kp} = 10^3 \text{ Pa}$,$1 \text{ cc} = 10^{-6} \text{ m}^3$)

The $P-V$ diagram of $2\,g$ of helium gas for a certain process $A \to B$ is shown in the figure. What is the heat given to the gas during the process $A \to B$ (in $,P_0V_0$)?

The $PV$ diagram shows four different possible reversible processes performed on a monatomic ideal gas. Process $A$ is isobaric (constant pressure). Process $B$ is isothermal (constant temperature). Process $C$ is adiabatic. Process $D$ is isochoric (constant volume). For which process(es) does the temperature of the gas decrease?