Question

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.

Answer 1

1. I shifts toward products and II shifts toward reactants.

Step-by-step explanation:

Hello,

In his case, since the reaction I) is endothermic (positive ∆H°) and the reaction II) is exothermic (negative ∆H°):

- In the first case, the energy is understood as a reactant, so if the temperature increases, heat is added so the reaction will shift rightwards (towards products).

- In the second case, the energy is understood as a product, so if the temperature increases, heat is added so the reaction will shift leftwards (towards reactants).

Therefore, the answer is:

1. I shifts toward products and II shifts toward reactants.

Best regards.