A thermodynamic system undergoes cyclic process $ABCDA $ as shown in figure. The work done by the system in the cycle is

In the $P-V$ diagram shown, the gas does $5\, J$ of work in isothermal process $ab$ and $4\,J$ in adiabatic process $bc$.   …. $J$ will be the change in internal energy of the gas in straight path $c$ to $a$ ?

A thermodynamic process is shown in the figure. The pressures and volumes corresponding to some points in the figure are :

${P_A} = 3 \times {10^4}Pa,\;{P_B} = 8 \times {10^4}Pa$ and ${V_A} = 2 \times {10^{ – 3}}{m^3},\;{V_D} = 5 \times {10^{ – 3}}{m^3}$

In process $AB$, $600 J$ of heat is added to the system and in process $BC, 200 J $ of heat is added to the system. The change in internal energy of the system in process $ AC$ would be …… $J$

Consider the following volume-temperature $( V – T )$ diagram for the expansion of $5$ moles of an ideal monoatomic gas.

Considering only $P-V$ work is involved, the total change in enthalpy (in Joule) for the transformation of state in the sequence $X \rightarrow Y \rightarrow Z$ is $\qquad$

[Use the given data: Molar heat capacity of the gas for the given temperature range, $C _{ v , m }=12 J K ^{-1} mol ^{-1}$ and gas constant, $R =8.3 J K ^{-1} mol ^{-1}$ ]

The above $P-V$ diagram represents the thermodynamic cycle of an engine, operating with an ideal monatomic gas. The amount of heat, extracted from the source in a single cycle is