Thermodynamic processes are indicated in the following diagram.
            
Match the following:

Column I		Column II
\(P\).	Process-I	\(\mathrm{a}\).	Adiabatic
\(Q\).	Process-II	\(\mathrm{b}\).	Isobaric
\(R\).	Process-III	\(\mathrm{c}\).	Isochoric
\(S\).	Process-IV	\(\mathrm{d}\).	Isothermal

1.	\(P \rightarrow \mathrm{a}, Q \rightarrow \mathrm{c}, R \rightarrow \mathrm{d}, S \rightarrow \mathrm{b}\)
2.	\(P \rightarrow \mathrm{c}, Q \rightarrow \mathrm{a}, R \rightarrow \mathrm{d}, S \rightarrow b\)
3.	\(P \rightarrow \mathrm{c}, Q \rightarrow \mathrm{d}, R \rightarrow \mathrm{b}, S \rightarrow \mathrm{a}\)
4.	\(P \rightarrow \mathrm{c}, Q \rightarrow \mathrm{d}, R \rightarrow \mathrm{b}, S \rightarrow \mathrm{a}\)

An ideal gas goes from state \(A\) to state \(B\) via three different processes, as indicated in the \(P\text-V\) diagram. If \(Q_1,Q_2,Q_3\)${\mathrm{}}_{}$ indicates the heat absorbed by the gas along the three processes and \(\Delta U_1, \Delta U_2, \Delta U_3\) indicates the change in internal energy along the three processes respectively, then:

In thermodynamic processes, which of the following statements is not true?

The specific heat of a gas in an isothermal process is: 

Two identical samples of a gas are allowed to expand, (i) isothermally and (ii) adiabatically. The work done will be:

In an adiabatic expansion of a gas, if the initial and final temperatures are \(T_1\) and \(T_2\), respectively, then the change in internal energy of the gas is:
1. \(\frac{nR}{\gamma-1}(T_2-T_1)\)
2. \(\frac{nR}{\gamma-1}(T_1-T_2)\)
3. \(nR ~(T_1-T_2)\)
4. Zero

In a cyclic process, the internal energy of the gas:

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 following figures, four curves A, B, C and D, are shown. The curves are:

For the indicator diagram given below, which of the following is not correct?