Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide as shown below. caco3(s) cao(s) + co2(g) the kp for this reaction is 1.16 at 800°c. a 5.00 l vessel containing 10.0 g of caco3(s) was evacuated to remove the air, sealed, and then heated to 800°c. ignoring the volume occupied by the solid, what will be the mass of the solid in the vessel once equilibrium is reached?

Explanation:

The balanced equation is

CaCO₃(s) ⇌ CaO(s) + CO₂(g); Kp = 1.16

Calculate Kc

T= 800 °C = 1073 K; Δn= 1

Equilibrium concentration of CO₂

Moles of CO₂ formed

Moles of CaCO₃ used up

Moles of CaCO₃ used up = moles of CO₂ formed = 6.155 × 10⁻⁴ mol

Mass of CaCO₃ used up

Moles of CaO formed

Moles of CaO formed = moles of CO₂ formed = 6.155 × 10⁻⁴ mol

Mass of CaO formed

Mass of solid at equilibrium

m = 10.0 g – 0.0616 g + 0.0345 g = 10.0 g

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