Chemical EquilibriumHard

Question

For the gaseous reaction: CO + H2O$\rightleftharpoons$CO2 + H2, the following thermodynamical data are given.

ΔHo300 K = – 41.0 kJ mol−1; ΔSo300 K = –0.04 kJ K−1 mol−1

ΔHo1200 K = – 33.0 kJ mol−1; ΔSo1200 K = –0.03 kJ K−1 mol−1

Assuming partial pressure of each component is 1 bar, the direction of spontaneous reaction is/are

Options

A.forward at 300 K.
B.forward at 1200 K.
C.backward at 300 K.
D.backward at 1200 K.

Solution

At 300K: ΔG° = (–41) – 300 × (–0.04) = –29 KJ/mol

Hence, the reaction is spontaneous in forward direction.

At 1200 K: ΔG° = (–33) – 1200 × (–0.03) = + 3 KJ/mol

Hence, the reaction is spontaneous in backward direction.

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