- 1(current)
Q. No.Refer to the given figure. Let \(\Delta U_1\) and \(\Delta U_2\) be the changes in internal energy of the system in processes \(A\) and \(B\). Then:
| 1. | \(\Delta U_1>\Delta U_2\) | 2. | \(\Delta U_1=\Delta U_2\) |
| 3. | \(\Delta U_1<\Delta U_2\) | 4. | \(\Delta U_1\neq\Delta U_2\) |
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| Assertion (A): | Internal energy of an ideal gas does not change when it is taken through a cyclic process. |
| Reason (R): | Internal energy is a state function, and when the gas returns to the same state – it attains the same value independent of the process. |
Choose the correct option from the given ones:
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 3. | (A) is True but (R) is False. |
| 4. | (A) is False but (R) is True. |
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The ratio of the temperatures at \(B,A\) i.e., \(T_B/T_A\) equals:
1. \(2\)
2. \(\dfrac12\)
3. \(4\)
4. \(\dfrac14\)
In each of the four diagrams \((\mathrm a)\) to \((\mathrm d),\) the variation of pressure \(p\) with volume \(V\) is shown as a closed path. The gas undergoes a cyclic process along the path \(ABCDA.\) What will be the net change in the internal energy of the gas after completing one full cycle in each case?
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| \((\mathrm a)\) | \((\mathrm b)\) |
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| \((\mathrm c)\) | \((\mathrm d)\) |
| 1. | The change in internal energy is zero in all four cases. |
| 2. | Positive in cases \((\mathrm a),(\mathrm b)\) and \((\mathrm c),\) but zero in case \((\mathrm d).\) |
| 3. | Negative in cases \((\mathrm a),(\mathrm b)\) and \((\mathrm c),\) but zero in the case \((\mathrm d).\) |
| 4. | Positive in all cases from \((\mathrm a)\) to \((\mathrm d).\) |
If \(Q\), \(E\), and \(W\) denote respectively the heat added, the change in internal energy, and the work done in a closed cycle process, then:
| 1. | \(W=0\) | 2. | \(Q=W=0\) |
| 3. | \(E=0\) | 4. | \(Q=0\) |
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| 1. | \(2 {PV}\) | 2. | \(4{PV}\) |
| 3. | \(\dfrac{1}{2}{PV}\) | 4. | \(PV\) |
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- 1(current)
Q. No.
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