The work done during reversible isothermal expansion of one mole of hydrogen gas at 25oC from a pressure of 20 atm to 10 atm is:
(Given R = 2.0 cal K-1 mol-1)
(Given R = 2.0 cal K-1 mol-1)
- 0 calorie
- -413.14 calories
- 413.14 calories
- 100 calories
The Correct Option is B
Solution and Explanation
1. For isothermal expansion, work done is calculated as:
\(W = -nRT \ln \frac{P_2}{P_1}\)
2. Substituting the given values:
\(W = -(1) \times (2.0) \times (298) \times \ln \left(\frac{10}{20}\right)\)
3. Simplify:
\(W = -596 \times \ln(0.5) = -596 \times (-0.693) \approx -413.14 \text{ calories}\).
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