196 The normal boiling point of Br2(l) is 58.8 ∘C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. a)...

Question

Question

196

The normal boiling point of Br2(l) is 58.8 ∘C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol.

a) When Br2(l) boils at its normal boiling point, does its entropy increase or decrease?

b) Calculate the value of ΔS when 1.50 mol of Br2(l) is vaporized at 58.8 ∘C.

ΔS=

(answer in J/K)

Answer 1

Answer #1

a)

entropy must be increased, since disorder and chaos is being increased. Besides, entropy is a function of temperature

b)

dS when n = 1.5 mol of Br2 is vaporized

dS = dH/T

dS = 29.6 kJ/mol / (58.8+273)K = 0.0892 kJ/molK * 1.5 mol = 0.1338 kJ/K

dS = 133.8 J/K

Answer 2

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