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 |
If a gas changes volume from 2 litres to 10 litres at a constant temperature of 300K, then the change in its internal energy will be:
1. | 12 J | 2. | 24 J |
3. | 36 J | 4. | 0 J |
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. | \(\frac{25 nγR}{\gamma - 1}\) |
In the \(P\text-V\) graph shown for an ideal diatomic gas, the change in the internal energy is:
1. | \(\frac{3}{2}P(V_2-V_1)\) | 2. | \(\frac{5}{2}P(V_2-V_1)\) |
3. | \(\frac{3}{2}P(V_1-V_2)\) | 4. | \(\frac{7}{2}P(V_1-V_2)\) |
If 3 moles of a monoatomic gas do 150 J of work when it expands isobarically, then a change in its internal energy will be:
1. | 100 J | 2. | 225 J |
3. | 400 J | 4. | 450 J |
If the ratio of specific heat of a gas at constant pressure to that at constant volume is , the change in internal energy of a mass of gas, when the volume changes from V to 2V at constant pressure, P is:
1. | 2. | PV | |
3. | 4. |
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. | \(5 \over 7\) |
The pressure in a monoatomic gas increases linearly from 4 atm to 8 atm when its volume increases from 0.2 m to 0.5 m. The increase in internal energy will be:
1. | 480 kJ | 2. | 550 kJ |
3. | 200 kJ | 4. | 100 kJ |