5 mole of an ideal gas expand reversibly from a volume of 8 dm3 to 80 dm3 at a temperature of 27°C. Calculate the change in entropy.
Correct answer: C. 95.73 JK-1
- A. 70.26 JK-1
- B. 82.55 JK-1
- C. 95.73 JK-1
- D. 107.11 JK-1
Explanation
To calculate the change in entropy of an ideal gas, we can use the formula:ΔS = nR ln(V2/V1)Given that 5 moles of an ideal gas expand reversibly from a volume of 8 dm³ to 80 dm³ at a temperature of 27°C, we can calculate the change in entropy as follows:ΔS = (5 mol) (8.314 J/mol K) log(80 dm³/8 dm³) = 5 mol x 8.314 J/mol K x 2.197 = 95.73 J/KThis means that Option C is the correct answer as it provides the accurate change in entropy. The other options are incorrect because they do not calculate the change in entropy correctly.
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Thermochemistry measures energy changes in chemical reactions and distinguishes exothermic from endothermic processes. Work covers systems, surroundings and state functions, internal energy, the first law of thermodynamics, enthalpy and Hess's law, including the sign conventions used when heat enters or leaves a system.
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