Suppose 1.00 kg of water at 42.5° C is placed in contact with 1.00 kg of water at 19.5° C. (a) What is the change in energy (in joules) of the hot water due to the heat transfer when it is placed in contact with the cold water and allowed to reach equilibrium? (b) What is the change in entropy in joules per kelvin due to this heat transfer?
Suppose 1.00 kg of water at 42.5° C is placed in contact with 1.00 kg of water at 19.5° C. (a) What is the change in energy (in joules) of the hot water due to the heat transfer when it is placed in contact with the cold water and allowed to reach equilibrium? (b) What is the change in entropy in joules per kelvin due to this heat transfer?
Chapter4: The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 76AP: Suppose 20 g of ice at 0 is added to 300 g of water at 60 . What is the total change in entropy of...
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Suppose 1.00 kg of water at 42.5° C is placed in contact with 1.00 kg of water at 19.5° C.
(a) What is the change in energy (in joules) of the hot water due to the
(b) What is the change in entropy in joules per kelvin due to this heat transfer?
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The answer to (a) is -ve but (b) isn't correct wether +ive or -ive. I'm not understanding (b).
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