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

        

1.	isothermal for A and D while adiabatic for B and C.
2.	adiabatic for A and C while isothermal for B and D.
3.	isothermal for A and B while adiabatic for C and D.
4.	isothermal for A and C while adiabatic for B and D.

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 a cyclic process, the internal energy of the gas:

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

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

The specific heat of a gas in an isothermal process is: 
1. Infinite
2. Zero
3. Negative
4. Remains constant

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

An ideal gas goes from state A to state B via three different processes, as indicated in the P-V diagram. If ${\mathrm{Q}}_1,$ ${\mathrm{Q}}_2,$ ${\mathrm{Q}}_3$ indicates the heat absorbed by the gas along the three processes and $∆{\mathrm{U}}_1,$ $∆{\mathrm{U}}_2,$ $∆{\mathrm{U}}_3$ indicates the change in internal energy along the three processes respectively, then:

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

A sample of \(0.1\) g of water at \(100^{\circ}\mathrm{C}\)$$ and normal pressure (\(1.013 \times10^5\) N m^–2) requires \(54\) cal of heat energy to convert it into steam at \(100^{\circ}\mathrm{C}\)$$. If the volume of the steam produced is \(167.1\) cc, then the change in internal energy of the sample will be:
1. \(104.3\) J
2. \(208.7\) J
3. \(42.2\) J
4. \(84.5\) J