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Q. No.The specific heat of a gas in an isothermal process is:
| 1. | Infinite | 2. | Zero |
| 3. | Negative | 4. | Remains constant |
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:
| 1. | \(\dfrac{2}{5}\) | 2. | \(\dfrac{2}{3}\) |
| 3. | \(\dfrac{1}{3}\) | 4. | \(\dfrac{2}{7}\) |
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:
| 1. | \(\dfrac{2}{5}\) | 2. | \(\dfrac{3}{5}\) |
| 3. | \(\dfrac{3}{7}\) | 4. | \(\dfrac{5}{7}\) |
One mole of an ideal monatomic gas undergoes a process described by the equation \(PV^3=\text{constant}.\) The heat capacity of the gas during this process is:
1. \(\frac{3}{2}R\)
2. \(\frac{5}{2}R\)
3. \(2R\)
4. \(R\)
(where symbols have their usual meanings)
1. \(C_P = \frac{\gamma R}{\gamma-1 }\)
2. \(C_P-C_V= R\)
3. \(\Delta U = \frac{P_fV_f-P_iV_i}{1-\gamma}\)
4. \(C_V = \frac{R}{\gamma-1 }\)
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:
| 1. | \(∆U_1 > ∆U_2\) | 2. | \(∆U_1 < ∆U_2\) |
| 3. | \(∆U_1 = ∆U_2\) | 4. | \(∆U_1 \leq ∆U_2\) |
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Q. No.
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