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Q. No.1. \(\Delta \mathrm{q} \neq 0, \Delta \mathrm{~T}=0, \mathrm{~W}=0 \)
2. \(\Delta \mathrm{q}=0, \Delta \mathrm{~T}=0, \mathrm{~W}=0 \)
3. \(\Delta \mathrm{q}=0, \Delta \mathrm{~T}<0, \mathrm{~W} \neq 0 \)
4. \(\Delta \mathrm{q}=0, \Delta \mathrm{~T} \neq 0, \mathrm{~W}=0\)
Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be:
1. 3 Joules
2. 9 Joules
3. Zero
4. Infinite
The work done during the expansion of a gas from a volume of 4 dm3 to 6 dm3 against a constant external pressure of 3 atm is:
1. –608 J
2. +304 J
3. –304 J
4. –6.00 J
The molar heat capacity of water at constant pressure, C, is 75 JK–1 mol–1. When 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of the water is:
| 1. | 1.2 K | 2. | 2.4 K |
| 3. | 4.8 K | 4. | 6.6 K |
In a closed insulated container a liquid is stirred with a paddle to increase the temperature. The correct option regarding this among the following is:
1. ∆E = W ≠ 0, q = 0
2. ∆E = W = q ≠ 0
3. ∆E = 0, W = q ≠ 0
4. W = 0 , ∆E = q ≠ 0
When 1 mol gas is heated at constant volume, the temperature is raised from 298 to 308 K. Heat supplied to the gas is 500 J. The correct statement among the following is:
1. q = w = 500 J, ∆U = 0
2. q = ∆U = 500 J, w = 0
3. q =0, w = 500 J, ∆U = 0
4. ∆U = 0, q = w = – 500 J
One mole of an ideal gas at 300 K is expanded isothermally from an initial volume of 1 litre to 10 litres. The ∆E for this process is:
(R = 2 cal. )
| 1. | 1381.1 cal. | 2. | Zero |
| 3. | 163.7 cal. | 4. | 9 lit. atm |
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Q. No.
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