The reaction,MgO(s) + C(s) → Mg(s) + CO(g), for which ΔrH° = +491.1 kJ mol–1 and ΔrS° = 198.0 JK–1 mol–1, is not feasible at 298 K. Temperature above which reaction will be feasible is

Engineering

Chemistry

Gibbs Free Energy Entropy and Spontaneity

Question

The reaction,

MgO(s) + C(s) → Mg(s) + CO(g), for which Δ_rH° = +491.1 kJ mol^–1 and Δ_rS° = 198.0 JK^–1 mol^–1, is not feasible at 298 K. Temperature above which reaction will be feasible is

2040.5 K

2480.3 K

1890.0 K

2380.5 K

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In order to be spontaneous ΔG° should be –ve

ΔG° = ΔH° – TΔS°

0 = 491.1 × 10³ – T × 198

$T = \frac{491100}{198} = 2480$

If temp is above 2480 K, the reaction will be spontaneous.