An ideal gas goes from A to B via two processes, l and ll, as shown. If and are the changes in internal energies in processes I and II, respectively, then (\(P:\) pressure, \(V:\) volume)
1. | ∆U1 > ∆U2 | 2. | ∆U1 < ∆U2 |
3. | ∆U1 = ∆U2 | 4. | ∆U1 ≤ ∆U2 |
The incorrect relation is:
(where symbols have their usual meanings)
1.
2.
3.
4.
If n moles of an ideal gas is heated at a constant pressure from 50°C to 100°C, the increase in the internal energy of the gas will be: \(\left(\frac{C_{p}}{C_{v}} = \gamma\ and\ R = gas\ constant\right)\)
1. \(\frac{50 nR}{\gamma - 1}\)
2. \(\frac{100 nR}{\gamma - 1}\)
3. \(\frac{50 nγR}{\gamma - 1}\)
4. \(\frac{25 nγR}{\gamma - 1}\)
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. | \(2 \over 5\) | 2. | \(3 \over 5\) |
3. | \(3 \over 7\) | 4. | \(5 \over 7\) |
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.
2.
3.
4.
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. | \(2 \over 5\) | 2. | \(2 \over 3\) |
3. | \(1 \over 3\) | 4. | \(2 \over 7\) |