A gas undergoes an isothermal process. The specific heat capacity of the gas in the process is:
1. | infinity | 2. | \(0.5\) |
3. | zero | 4. | \(1\) |
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 \(\mathrm{A}\) to state \(\mathrm{B}\) will be:
1. | \(2 \over 5\) | 2. | \(2 \over 3\) |
3. | \(1 \over 3\) | 4. | \(2 \over 7\) |
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. \(R\)
1. | \(\frac{R}{\gamma -1}\) | 2. | \(\frac{\gamma -1}{R}\) |
3. | \(\gamma R \) | 4. | \(\frac{\left ( \gamma -1 \right )R}{\left ( \gamma +1 \right )}\) |
The molar specific heat at a constant pressure of an ideal gas is \(\dfrac{7}{2}R.\) The ratio of specific heat at constant pressure to that at constant volume is:
1. | \(\dfrac{7}{5}\) | 2. | \(\dfrac{8}{7}\) |
3. | \(\dfrac{5}{7}\) | 4. | \(\dfrac{9}{7}\) |
When volume changes from \(V\) to \(2V\) at constant pressure(\(P\)), the change in internal energy will be:
1. \(PV\)
2. \(3PV\)
3. \(\frac{PV}{\gamma -1}\)
4. \(\frac{RV}{\gamma -1}\)
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 |