Entropy and the Second Law of Thermodynamics
Chapter , Problem 25E(choose chapter or problem)
The normal boiling point of \(\operatorname{Br}_{2}(I)\) is \(58.8^{0} \mathrm{C}\), and its molar enthalpy of vaporization is \(\Delta H_{v a p}=29.6 \mathrm{~kJ} / \mathrm{mol}\). (a) When \(\operatorname{Br}_{2}(I)\) boils at its normal boiling point, does its entropy increase or decrease? (b) Calculate the value of \(\Delta S\) when mol of \(\operatorname{Br}_{2}(I)\) is vaporized at \(58.8^{0} \mathrm{C}\)
Equation transcription:
Text transcription
\operatorname{Br}_{2}(I):
58.8^{0} \mathrm{C}
\Delta H_{v a p}=29.6 \mathrm{~kJ} / \mathrm{mol}
\Delta S
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