A solid copper block at 130°C is placed in a massive open atmosphere at 32°C. The block reversibly l — Thermodynamics and Thermochemistry Chemistry Question
Question
A solid copper block at 130°C is placed in a massive open atmosphere at 32°C. The block reversibly loses 340 J of heat to the surroundings. Assuming temperatures remain momentarily constant, what is the total entropy change of the universe for this initial step?
Answer: A
💡 Solution & Explanation
Absolute temperatures: $T_{sys} = 403 \text{ K}$, $T_{surr} = 305 \text{ K}$. System entropy $\Delta S_{sys} = -340 / 403 \approx -0.84$ J/K. Surrounding entropy $\Delta S_{surr} = +340 / 305 \approx +1.11$ J/K. Universe entropy $\Delta S_{univ} = -0.84 + 1.11 = +0.27$ J/K.
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