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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