Q. No.A refrigerator works between and . It is required to remove 600 calories of heat every second to keep the temperature of the refrigerated space constant. The power required will be:
(Take, 1 cal= 4.2 Joules)
1. 23.65 W
2. 236.5 W
3. 2365 W
4. 2.365 W
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A monoatomic gas at a pressure \(P\), having a volume \(V\), expands isothermally to a volume \(2V\) and then adiabatically to a volume \(16V\). The final pressure of the gas is: \(\left(\text{Take:}~ \gamma = \frac{5}{3} \right)\)
| 1. | \(64 ~P\) | 2. | \(32~P\) |
| 3. | \(\frac{P}{64}\) | 4. | \(16~P\) |
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A thermodynamic system undergoes a cyclic process \(ABCDA\) as shown in Fig. The work done by the system in the cycle is:
1. \( P_0 V_0 \)
2. \( 2 P_0 V_0 \)
3. \( \frac{P_0 V_0}{2} \)
4. zero
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| 1. | \(1000~\text{J}\) | 2. | zero |
| 3. | \(-2000~\text{J}\) | 4. | \(2000~\text{J}\) |
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A Carnot engine whose sink is at \(300~\mathrm{K}\) has an efficiency of \(40\)%. By how much should the temperature of the source be increased to increase its efficiency by \(50\)% of its original efficiency?
| 1. | \(275~\mathrm{K}\) | 2. | \(325~\mathrm{K}\) |
| 3. | \(250~\mathrm{K}\) | 4. | \(380~\mathrm{K}\) |
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One mole of an ideal gas expands at a constant temperature of 300 K from an initial volume of 10 litres to a final volume of 20 litres.
The work done in expanding the gas is equal to:
(R = 8.31 J/mole-K)
1. 750 joules
2. 1728 joules
3. 1500 joules
4. 3456 joules
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The efficiency of an ideal heat engine (Carnot heat engine) working between the freezing point and boiling point of water is:
1. \(26.8\%\)
2. \(20\%\)
3. \(6.25\%\)
4. \(12.5\%\)
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The volume (\(V\)) of a monatomic gas varies with its temperature (\(T\)), as shown in the graph. The ratio of work done by the gas to the heat absorbed by it when it undergoes a change from state \(\mathrm{A}\) to state \(\mathrm{B}\) will be:
| 1. | \(2 \over 5\) | 2. | \(2 \over 3\) |
| 3. | \(1 \over 3\) | 4. | \(2 \over 7\) |
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The temperature inside a refrigerator (reversible process) is t2oC and the room temperature is t1oC. The amount of heat delivered to the room for each joule of electrical energy consumed, ideally, will be:
1.
2.
3.
4.
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A sample of \(0.1\) g of water at \(100^{\circ}\mathrm{C}\) and normal pressure (\(1.013 \times10^5\) N m–2) requires \(54\) cal of heat energy to convert it into steam at \(100^{\circ}\mathrm{C}\). If the volume of the steam produced is \(167.1\) cc,
then the change in internal energy of the sample will be:
1. \(104.3\) J
2. \(208.7\) J
3. \(42.2\) J
4. \(84.5\) J
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