1. | \(1.5\%\) | increases by
2. | \(1.5\%\) | decreases by
3. | \(\frac13\%\) | increases by
4. | \(\frac23\%\) | increases by
One mole of an ideal gas goes from an initial state \(A\) to the final state \(B\) with two processes. It first undergoes isothermal expansion from volume \(V\) to \(3V\) and then its volume is reduced from \(3V\) to \(V\) at constant pressure. The correct \((P-V)\) diagram representing the two processes is:
1. | 2. | ||
3. | 4. |
The ratio \(C_P/C_V=1.5\) for a certain ideal gas. The gas is taken at an initial pressure of \(2\) kPa and compressed suddenly to \(\frac14\) of its initial volume. The final pressure is:
1. \(\frac12\) kPa
2. \(4\) kPa
3. \(8\) kPa
4. \(16\) kPa
If heat is supplied to an ideal gas in an isothermal process,
1. | the internal energy of the gas will increase. |
2. | the gas will do positive work. |
3. | the gas will do negative work. |
4. | the said process is not possible. |
In thermodynamic processes which of the following statements is not true?
1. | In an adiabatic process, the system is insulated from the surroundings. |
2. | In an isochoric process, pressure remains constant. |
3. | In an isothermal process, the temperature remains constant. |
4. | In an adiabatic process \(PV^\gamma=\mathrm{constant}.\) |