The calcination of limestone CaCO₃(s) → CaO(s) + CO₂(g) ΔH ≈ +178 kJ·mol⁻¹ is to be…
CHEMISTRY · Single correct · A Level · Chemistry · Energetics · Energetics
Problem
The calcination of limestone
CaCO₃(s) → CaO(s) + CO₂(g) ΔH ≈ +178 kJ·mol⁻¹
is to be paired with the combustion of carbon monoxide to reduce the net energy demand:
CO(g) + ½ O₂(g) → CO₂(g) ΔH ≈ –283 kJ·mol⁻¹
Approximately how many moles of CO must be combusted per mole of CaCO₃ decomposed so that the overall enthalpy change is closest to zero?
(a) 0.80mol
(b) 0.60mol
(c) 1.00mol
(d) 0.50mol