Question on: JAMB Chemistry - 2009
C(s) + H2O(g) → H2(g) + CO2(g)
ΔG for the reaction above at 1300k is -43KJ. At this temperature, the reaction is
ΔG for the reaction above at 1300k is -43KJ. At this temperature, the reaction is
A
not feasible
B
at equilibrium
C
feasible
D
exothermic
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Correct Option: C
* The Gibbs free energy change (ΔG) determines the spontaneity of a reaction.
* A negative ΔG indicates that the reaction is spontaneous or feasible under the given conditions.
* Since the ΔG is -43 kJ at 1300 K, the reaction is feasible at that temperature.
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