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Q. No.The following figure shows two processes \(A\) and \(B\) for a gas. If \(\Delta Q_A\) and \( \Delta Q_B\) are the amount of heat absorbed by the system in two cases, and \(\Delta U_A\) and \(\Delta U_B\) are changes in internal energies, respectively, then:
| 1. | \( \Delta Q_A>\Delta Q_B,~ \Delta U_A>\Delta U_B \) |
| 2. | \( \Delta Q_A<\Delta Q_B,~ \Delta U_A<\Delta U_B \) |
| 3. | \( \Delta Q_A>\Delta Q_B, ~\Delta U_A=\Delta U_B \) |
| 4. | \( \Delta Q_A=\Delta Q_B, ~\Delta U_A=\Delta U_B \) |
Subtopic: Β First Law of Thermodynamics |
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A diatomic gas with rigid molecules undergoes expansion at constant pressure, performing \(10~\text{J}\) of work in the process. What is the amount of heat energy absorbed by the gas during this process?
1. \(35~\text{J}\)
2. \(40~\text{J}\)
3. \(25~\text{J}\)
4. \(30~\text{J}\)
Subtopic: Β First Law of Thermodynamics |
Β 63%
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For a system undergoing an isothermal process, heat energy is supplied to the system. Then,
Choose the correct option from the given ones:
| I. | Internal energy will increase. |
| II. | Internal energy will decrease. |
| III. | Work done by the system is positive. |
| IV. | Work done by the system is negative. |
| V. | Internal energy remains constant. |
Choose the correct option from the given ones:
| 1. | (I), (III), and (V) only | 2. | (II) and (IV) only |
| 3. | (III) and (V) only | 4. | (I), (IV), and (V) only |
Subtopic: Β First Law of Thermodynamics |
Β 85%
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The initial volume of \(1\) mole of a monoatomic gas is \(2\) litres. It is expanded isothermally to a volume of \(6\) litres. Change in internal energy of the gas is:
1. \(2R\)
2. \(4R\)
3. \(R\)
4. \(0\)
1. \(2R\)
2. \(4R\)
3. \(R\)
4. \(0\)
Subtopic: Β First Law of Thermodynamics |
Β 89%
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During an adiabatic process performed on a diatomic gas \(725\) J of work is done on the gas. The change in internal the energy of the gas is equal to:
1. \(495\) J
2. \(725\) J
3. \(225\) J
4. \(0\)
1. \(495\) J
2. \(725\) J
3. \(225\) J
4. \(0\)
Subtopic: Β First Law of Thermodynamics |
Β 91%
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When the amount of heat supplied to a gas in a system is equal to \(1000\) J, the system in return does \(200\) J of work on the surrounding. What would be the change in the internal energy of the gas?
1. \(800\) J
2. \(1200\) J
3. \(1000\) J
4. \(1100\) J
1. \(800\) J
2. \(1200\) J
3. \(1000\) J
4. \(1100\) J
Subtopic: Β First Law of Thermodynamics |
Β 76%
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A gas is compressed adiabatically. Which of the following statements is not correct?
| 1. | Internal energy is constant |
| 2. | Temperature increases |
| 3. | |Work done| = |change in internal energy| |
| 4. | Heat is not supplied to the system |
Subtopic: Β First Law of Thermodynamics |
Β 67%
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Q. No.
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