When heated, CaCO₃ decomposes into CaO and CO₂ according to the following equation: CaCO₃ (s) ⇌ CaO (s) + CO₂ (g) This is an endothermic reaction in which ∆H° = 178.3 kJ/mol and in which entropy increases, ∆S° = 159 J/mol･K. To what temperature (in °C) must CaCO₃ be heated in a closed container in order to produce CO₂ at an equilibrium pressure of 0.100 atm? (Assume ∆H° and ∆S° do not change appreciably with temperature).

Question

Chemistry

Peyton Boyd

14 February, 21:19

When heated, CaCO₃ decomposes into CaO and CO₂ according to the following equation: CaCO₃ (s) ⇌ CaO (s) + CO₂ (g) This is an endothermic reaction in which ∆H° = 178.3 kJ/mol and in which entropy increases, ∆S° = 159 J/mol･K. To what temperature (in °C) must CaCO₃ be heated in a closed container in order to produce CO₂ at an equilibrium pressure of 0.100 atm? (Assume ∆H° and ∆S° do not change appreciably with temperature).

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Answers (1)

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Damari Atkinson · Answer 1

T = 1,121K

Explanation:

At equilibrium,

∆H° = T∆S°

∆H° = 178.3, ∆S° = 159J/mol = 0.159kJ/mol

Substitute into above formula

178.3 = T * 0.159

T = 1,121K