When an ideal diatomic gas is heated at constant pressure, the fraction of the heat energy supplied which increases the internal energy of the gas, is

In the diagrams $(i)$ to $(iv)$ of variation of volume with changing pressure is shown. A gas is taken along the path $ABCD. $ The change in internal energy of the gas will be

An ideal gas of mass $m$ in a state $A$ goes to another state $B$ via three different processes as shown in figure. If $Q_{1}, Q_{2}$ and $Q_{3}$ denote the heat absorbed by the gas along the three paths, then

A $P-T$ graph is shown for a cyclic process. Select correct statement regarding this

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, $R =8.3 J K ^{-1} mol ^{-1}$ ]