Problem 30E
(a) Calculate the change in entropy when 1.00 mol of
Step-by-Step Solution:
Solution 30E a) The way we have defined temperature is, dS = 1 --------------------(1) dQ T dS = dQ / T . So the change in entropy is the change in heat divided by the boiling point. For water, T = 100 C = 373 K . The heat required to vaporize 1 mol of liquid water is, Q = mL =V18 g × 2265000 J /kg = 0.018 × 2265000 = 40.77 KJ = 40770 jules. The change in entropy is, dS = 40770 / 373 = 109.30 b) Step 1: For liquid nitrogen, Boiling temperature is T = 77.34 K . Heat required to vaporize 1 mol, Q = mL = 28g × 201000 J/kg = 0.028 × 201000 = 5628 jules. V So, the change in entropy is, dS = 5628 / 77.34 = 73.09
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Chapter 20, Problem 30E is Solved
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