- 1(current)
Q. No.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 |
(Use R = 8.314 J K–1 mol–1)
| 1. | 1260 J | 2. | 2520 J |
| 3. | 5040 J | 4. | 0 J |
An ideal gas expands isothermally at 300 K from a volume of 10⁻³ m³ to 10⁻² m³ against a constant
external pressure of 10⁵ N m⁻². Calculate the work associated with this expansion using the chemistry sign convention.
| 1. | \(+270 ~kJ\) | 2. | \(–900 ~J\) |
| 3. | \(+900 ~kJ\) | 4. | \(–900~ kJ\) |
A gas is allowed to expand in a well insulated container against a constant external pressure of 2.5 atm from an initial volume of 2.50 L to a final volume of 4.50 L. Determine the change in internal energy U of the gas:
| 1. | +500 J | 2. | -500 J |
| 3. | -506 J | 4. | +515 J |
A gas is allowed to expand in a well-insulated container against a constant external pressure of 2.5atm from an initial volume of 2.50 L to a final volume of 4.50L. The change in internal energy U of the gas in joules will be:
| 1. | –500J | 2. | –505J |
| 3. | –506J | 4. | –508J |
- 1(current)
Q. No.
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