The value of ΔG° for the reaction CO(g) + H₂O(g) ⇄ CO₂(g) + H₂(g), when ΔH° = -41.0 kJ/mol and ΔS° = -42.3 J/K*mol, at 25.0°C and 1 atm, is -28.40 kJ/mol.
The reaction is:
CO(g) + H₂O(g) ⇄ CO₂(g) + H₂(g) (1)
Gibbs free energy for reaction (1) is given by:
[tex] \Delta G^{\circ} = \Delta H^{\circ} - T\Delta S^{\circ} [/tex]
Where:
ΔH°: is the enthalpy of the reaction = -41.0 kJ/mol
ΔS°: is the entropy of the reaction = -42.3 J/K*mol
T: is the temperature = 25.0 °C = 298 K
The value of ΔG° is:
[tex] \Delta G^{\circ} = \Delta H^{\circ} - T\Delta S^{\circ} = -41.0 kJ/mol - 298 K(-42.3 \frac{J}{K*mol}*\frac{1 kJ}{1000 J}) = -28.40 kJ/mol [/tex]
Therefore, the value of ΔG° is -28.40 kJ/mol.
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