A dish containing 145 g of water at 54.0 degrees Celsius is put in a refrigerator...
A dish containing 145 g of water at 54.0 degrees Celsius is put in a refrigerator to cool. It is removed when the temperature ofthe water is 5.50 degrees Celsius. (Specific heat H2O(l)=4.184 j/gC.
a) how much heat (in KJ) does the water lose?
b) Describe how the entropy of the system changes in this process?
Homework Answers
a). Heat Lost by Water= 29.424 kJ
b). Entropy of the system DECREASES. Because, Entropy is the measurement of randomness of a system and as temperature of water is reduced, the randomness of the system will reduce.Hence entropy reduces.
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