Stuart Clarke
10/16/2023 · High School

3. A 25 kg iron block initially at \( 140^{\circ} \mathrm{C} \) is quenched in a rigid and well insulated tank that contains 100 kg of water at \( 18^{\circ} \mathrm{C} \). Assuming the water that vaporizes during the process condenses back in the tank, determine the total entropy change during this process.

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The total entropy change during the process is the sum of the entropy changes for the iron block and the water. After calculations, the entropy change for the iron block is approximately \( \Delta S_{Fe} = 25 \cdot 450 \cdot \ln\left(\frac{302.15}{413.15}\right) \) and for the water, \( \Delta S_{H2O} = 100 \cdot 4186 \cdot \ln\left(\frac{302.15}{291.15}\right) \). Therefore, the total entropy change is \( \Delta S_{total} = \Delta S_{Fe} + \Delta S_{H2O} \).

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