At 298 K the decomposition of solid calcium carbonate proceeds according to
CaCO₃(s) ⇌ CaO(s) + CO₂(g)
The standard Gibbs free-energy change for the reaction is ΔG° = +130.7 kJ·mol⁻¹. Assume ideal-gas behavior for CO₂. The universal gas constant is R = 8.314 J·mol⁻¹·K⁻¹.
(a) Calculate the equilibrium constant K for the reaction at 298 K. Express your answer in scientific notation.
(b) Determine log₁₀K (base-10 logarithm) for the equilibrium constant you obtained in part (a).
(c) Interpret the magnitude of K in terms of the relative amounts of CaCO₃(s), CaO(s), and CO₂(g) that would be present at equilibrium in a closed container at 298 K.