A 1.00-kg iron horseshoe is taken from a forge at 900°C and dropped into 4.00 kg of water at 10.0°C. Assuming that no energy is lost by heat to the surroundings, determine the total entropy change of the horseshoe-plus-water system. (Suggestion: Note that dQ = mc dT.)

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Q: Compute the entropy change of 5 g of water at 100 °C as it changes to steam at 100 °C.

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A: Heat 1.6 x 105 J Initial temperature = 20 C Entropy increases = 480 J/K

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A: Change in enteopy of a gasS2-S1=mcvPnT2T1+ mR ln V2V1

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Q: When 1.60 x 105 J of heat transfer occurs into a meat pie initially at 20.0°C, Its entropy increases…

A: solution as