Predict whether the equilibria I) CH4(g) + H2O(g) ⇀↽ CO(g) + 3 H2(g), ∆H◦ = +206 kJ II) 2 SO2(g) + O2 ⇀↽ 2 SO3(g), ∆H◦ = −198 kJ

Question

3 years ago

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Predict whether the equilibria I) CH4(g) + H2O(g) ⇀↽ CO(g) + 3 H2(g), ∆H◦ = +206 kJ II) 2 SO2(g) + O2 ⇀↽ 2 SO3(g), ∆H◦ = −198 kJ

will shift toward products or reactants with a temperature increase. 1. I shifts toward products and II shifts toward reactants. 2. Unable to determine 3. Both I and II shift toward products.

Chemistry

1 answer:

Dima020 [189] · Answer 1 · 2022-06-05T07:28:45+03:00

Answer:

(1) I shifts toward product and II shifts toward reactant.

Explanation:

Increasing the temperature of an endothermic reaction (∆H is positive) shifts the equilibrium position to the right thus favoring product formation.

Increasing the temperature of an exothermic reaction (∆H is negative) shifts the equilibrium position to the left thus favoring the backward reaction.