2H2(g) + O2(g) ⇌ 2H2O(g) ΔH = -ve
wha...
2H2(g) + O2(g) ⇌ 2H2O(g) ΔH = -ve
what happens to the equilibrium constant of the reaction above if the temperature is increased?
it is unaffected
it becomes zero
it decrease
it increase
Correct answer is C
This given equation shows the forward reaction is exothermic, which means an increase in temperature will cause the equilibrium position to shift to left to favor reactant formation, i.e K decreases
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