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.

Question

Taryn Prince

Chemistry

25 July, 18:54

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.

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Answers (1)

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Natalia Case · Answer 1

(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.