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What is the molar entropy of a pure crystal at 0 K, and what is the significance of the answer?
Ch.18 - Free Energy and Thermodynamics
Chapter 18, Problem 4
A reaction has ΔH°rxn = -112 kJ and ΔS°rxn = 354 J/K. At what temperature is the change in entropy for the reaction equal to the change in entropy for the surroundings?
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Identify the relationship between the change in entropy for the system (ΔS°_rxn) and the surroundings. The change in entropy for the surroundings (ΔS_surroundings) is given by the formula ΔS_surroundings = -ΔH°_rxn / T.
Set the change in entropy for the system equal to the change in entropy for the surroundings: ΔS°_rxn = -ΔH°_rxn / T.
Rearrange the equation to solve for the temperature (T): T = -ΔH°_rxn / ΔS°_rxn.
Substitute the given values into the equation. Remember to convert ΔH°_rxn from kJ to J by multiplying by 1000, so ΔH°_rxn = -112,000 J.
Calculate the temperature (T) using the rearranged equation with the substituted values.
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