The figure shows the \((P\text-V)\) diagram of an ideal gas undergoing a change of state from \(A\) to \(B\). Four different paths \(\mathrm{I, II, III}\) and \(\mathrm{IV}\), as shown in the figure, may lead to the same change of state.
(a) | The change in internal energy is the same in cases \(\mathrm{IV}\) and \(\mathrm{III}\) but not in cases \(\mathrm{I}\) and \(\mathrm{II}\). |
(b) | The change in internal energy is the same in all four cases. |
(c) | Work done is maximum in case \(\mathrm{I}\). |
(d) | Work done is minimum in case \(\mathrm{II}\). |
Which of the following options contains only correct statements?
1. (b), (c), (d)
2. (a), (d)
3. (b), (c)
4. (a), (c), (d)
Work done during the given cycle is:
1. 4
2. 2
3.
4.
A given mass of gas expands from state A to state B by three paths, 1, 2 and 3, as shown in the figure. If respectively be the work done by the gas along the three paths, then:
1. | W1 > W2 > W3 | 2. | W1 < W2 < W3 |
3. | W1 = W2 = W3 | 4. | W1 < W2 = W3 |
The pressure-temperature (P-T) graph for two processes, A and B, in a system is shown in the figure. If and are work done by the gas in process A and B respectively, then:
1. | \(W_{1}\) = \(W_{2}\) | 2. | \(W_{1}\) < \(W_{2}\) |
3. | \(W_{1}\) > \(W_{2}\) | 4. | \(W_{1}\) = \(-W_{2}\) |
The pressure of a monoatomic gas increases linearly from N/m2 to N/m2 when its volume increases from 0.2 m3 to 0.5 m3. The work done by the gas is:
1.
2.
3.
4.
Two identical samples of a gas are allowed to expand, (i) isothermally and (ii) adiabatically. Work done will be:
1. | more in the isothermal process. |
2. | more in the adiabatic process. |
3. | equal in both processes. |
4. | none of the above. |
\(0.04\) mole of an ideal monatomic gas is allowed to expand adiabatically so that its temperature changes from \(800~\text{K}\) to \(500~\text{K}\). The work done during expansion is nearly equal to:
1. | \(129.6\) J | 2. | \(-129.6\) J |
3. | \(149.6\) J | 4. | \(-149.6\) J |
1. | \(1000~\text{J}\) | 2. | zero |
3. | \(-2000~\text{J}\) | 4. | \(2000~\text{J}\) |