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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. | \(\Delta U_1\neq\Delta U_2\) |
Subtopic: Basic Terms |
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In a certain process, \(33.5\) kJ is furnished to the system while the system does \(6\) kJ of work. What is the change in the internal energy of the system?
1. \(39.5\) kJ
2. \(33.5\) kJ
3. \(27.5\) kJ
4. \(6\) kJ
1. \(39.5\) kJ
2. \(33.5\) kJ
3. \(27.5\) kJ
4. \(6\) kJ
Subtopic: First Law of Thermodynamics |
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A fixed mass of an ideal gas undergoes a change in which it is supplied with \(3500\) J of thermal energy. At the same time, this gas does \(3500\) J of work on its surroundings. Which type of change does the gas undergo during this time?
| 1. | adiabatic | 2. | isothermal |
| 3. | isochoric | 4. | isomeric |
Subtopic: First Law of Thermodynamics |
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Consider the following statements and select the correct option.
| Statement (A): | Heat is not a state function. |
| Statement (B): | Heat supplied to a system is a path function. |
| 1. | Both statements (A) and (B) are True. |
| 2. | Both statements (A) and (B) are False. |
| 3. | Only statement (A) is True. |
| 4. | Only statement (B) is True. |
Subtopic: Basic Terms |
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One mole of a diatomic ideal gas undergoes a cyclic process \(ABC\) as shown in the figure. The process \(BC\) is adiabatic. The temperatures at \(A,\) \(B,\) and \(C\) are \(400\) K, \(800\) K, and \(600\) K respectively. Choose the correct statement:
| 1. | The change in internal energy in the process \(BC\) is \(-500R.\) |
| 2. | The change in internal energy in the whole cyclic process is \(250R.\) |
| 3. | The change in internal energy in the process \(CA\) is \(700R.\) |
| 4. | The change in internal energy in the process \(AB\) is \(-350R.\) |
Subtopic: Cyclic Process |
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If \(\Delta Q\) is the heat flowing out of a system, \(\Delta W\) is the work done by the system on its surroundings, and \(\Delta U\) is the decrease in internal energy of the system, then the first law of thermodynamics can be stated as:
| 1. | \(\Delta Q=\Delta U+\Delta W\) |
| 2. | \(\Delta U=\Delta Q+\Delta W\) |
| 3. | \(\Delta U=\Delta Q-\Delta W\) |
| 4. | \(\Delta U+\Delta Q+\Delta W=0\) |
Subtopic: First Law of Thermodynamics |
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\(1\) mole of rigid diatomic gas performs a work of \(\dfrac{Q}{5}\) when heat \(Q\) is supplied to it. Change in internal energy of the gas is:
| 1. | \(\dfrac{4Q}{5}\) | 2. | \(\dfrac{3Q}{5}\) |
| 3. | \(\dfrac{Q}{5}\) | 4. | \(\dfrac{2Q}{5}\) |
Subtopic: First Law of Thermodynamics |
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The internal energy change in a system that has absorbed \(2\) kcal of heat and done \(500\) J of work is:
1. \(8900\) J
2. \(6400\) J
3. \(5400\) J
4. \(7900\) J
Subtopic: First Law of Thermodynamics |
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A thermodynamic process involving a system takes place with \(100\) J of heat being rejected to the environment and an increase of \(20\) J of internal energy. Then,
| 1. | work done by the system is \(120\) J. |
| 2. | work done on the system is \(120\) J. |
| 3. | work done by the system is \(80\) J. |
| 4. | work done on the system is \(80\) J. |
Subtopic: First Law of Thermodynamics |
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The internal energy of a gas is given by \(U=2pV.\) The gas expands from \(100\) cc to \(200\) cc against a constant pressure of \(10^{5}\) Pa. The heat absorbed by the gas is:
1. \(10\) J
2. \(20\) J
3. \(30\) J
4. \(40\) J
Subtopic: First Law of Thermodynamics |
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