- 1(current)
Q. No.The work done during reversible isothermal expansion of one mole of hydrogen gas at 25°C from a pressure of 20 atmosphere to a pressure of 10 atmosphere is :
(Given R = 2.0 cal K–1 mol–1)
(Given R = 2.0 cal K–1 mol–1)
| 1. | –413.14 calories | 2. | 413.14 calories |
| 3. | 100 calories | 4. | 0 calorie |
Subtopic: First Law of Thermodynamics |
71%
Level 2: 60%+
NEET - 2024
Hints
Choose the correct statement for the work done in the expansion and heat absorbed or released when 5 liters of an ideal gas at 10 atmospheric pressure isothermally expands into a vacuum until the volume is 15 liters:
| 1. | Both the heat and work done will be greater than zero. |
| 2. | Heat absorbed will be less than zero and work done will be positive. |
| 3. | Work done will be zero and heat absorbed or evolved will also be zero. |
| 4. | Work done will be greater than zero and heat absorbed will remain zero. |
Subtopic: First Law of Thermodynamics |
62%
Level 2: 60%+
NEET - 2024
Hints
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
Subtopic: First Law of Thermodynamics |
73%
Level 2: 60%+
NEET - 2022
Hints
One mole of an ideal gas at 300 K is expanded isothermally from 1 L to 10 L volume. \(\Delta U\) for this process is:
(Use R = 8.314 J K–1 mol–1)
(Use R = 8.314 J K–1 mol–1)
| 1. | 1260 J | 2. | 2520 J |
| 3. | 5040 J | 4. | 0 J |
Subtopic: First Law of Thermodynamics |
80%
Level 1: 80%+
NEET - 2022
Hints
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. | \(–900~ kJ\) |
Subtopic: First Law of Thermodynamics |
72%
Level 2: 60%+
NEET - 2019
Hints
- 1(current)
Q. No.
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