Question

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).

Answer 1

Answer:

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