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Q. No.What is the amount of work done by an ideal gas, if the gas expands isothermally from \(10^{-3}~m^3\) to \(10^{-2}~m^3\) at \(300~K\)against a constant pressure of \(10^{5}~Nm^{-2}\)?
| 1. | \(+270 ~kJ\) | 2. | \(–900 ~J\) |
| 3. | \(+900 ~kJ\) | 4. | \(–900~ kJ\) |
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
The work done when 1 mole of gas expands reversibly and isothermally from a pressure of 5 atm to 1 atm at 300 K is:
[Given: log 5 = 0.6989 and R = 8.314 J K-1 mol-1 ]
1. Zero J
2. 150 J
3. +4014.6 J
4. -4014.6 J
When 1 g H2 gas at S.T.P is expanded to twice its initial volume, then the work done is:
1. 22.4 L atm
2. 5.6 L atm
3. 11.2 L atm
4. 44.8 L atm
Two litres of an ideal gas at a pressure of 10 atm expands isothermally at 25 °C into a vacuum until its total volume is 10 litres. The amount of heat absorbed during expansion is:
1. 80 J
2. -80 J
3. Zero
4. 50 J
| Column-I (Process) |
Column-II (Expression)
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| a. | No heat is absorbed by the system from the surroundings, but work (w) is done on the system. | i. | ∆U = q – w, closed system. |
| b. | No work is done on the system, but q amount of heat is taken out from the system and given to the surroundings. | ii. | ΔU=Wad, for an adiabatic wall. |
| c. | w amount of work is done by the system and q amount of heat is supplied to the system. | iii. | ∆U = –q, thermally conducting walls. |
| 1. | a = i; b = ii; c = iii | 2. | a = ii; b = i; c = iii |
| 3. | a = ii; b = iii; c = i | 4. | a = iii; b = ii; c = i |
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