- 1(current)
Q. No.A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 37.0ºC. As it does so, it absorbs 208 J of heat. The values of q and w for the process will be-
(R = 8.314 J/mol K) (ln 7.5 = 2.01)
| 1. | q = +208 J, w = -208 J | 2. | q = -208 J, w = -208 J |
| 3. | q = -208 J, w = + 208 J | 4. | q = +208 J, w = + 208 J |
Subtopic: First Law of Thermodynamics |
82%
Level 1: 80%+
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
For the graph given below, it can be concluded that work done during the process shown will be-
| 1. | Zero | 2. | Negative |
| 3. | Positive | 4. | Cannot be determined |
Subtopic: First Law of Thermodynamics |
69%
Level 2: 60%+
Hints
Determine \(\Delta U\) for the process where, one mole of an ideal gas at 300 K is expanded isothermally from 1 L to 10 L volume:
(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
- 1(current)
Q. No.
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