An ideal gas goes from \(A\) to \(B\) via two processes, \(\mathrm{I}\) and \(\mathrm{II},\) as shown. If \(\Delta U_1\) and \(\Delta U_2\) are the changes in internal energies in processes \(\mathrm{I}\) and \(\mathrm{II},\) respectively,  (\(P:\) pressure, \(V:\) volume) then:

If \(n\) moles of an ideal gas is heated at a constant pressure from \(50^\circ\text C\) to \(100^\circ\text C,\) the increase in the internal energy of the gas will be:
\(\left(\frac{C_{p}}{C_{v}} = \gamma\   ~\text{and}~\   R = \text{gas constant}\right)\)

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:

Two cylinders contain the same amount of an ideal monoatomic gas. The same amount of heat is given to two cylinders. If the temperature rise in cylinder A is T₀, then the temperature rise in cylinder B will be:

1. $\frac{4}{3}{\mathrm{T}}_0$

2. $2{\mathrm{T}}_0$

3. $\frac{{\mathrm{T}}_0}{2}$

4. $\frac{5}{3}{\mathrm{T}}_0$

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

The volume \((V)\) of a monatomic gas varies with its temperature \((T),\) as shown in the graph. The ratio of work done by the gas to the heat absorbed by it when it undergoes a change from state \(A\) to state \(B\) will be: