A. ?G° = 141 . 8 kJ?/?mol. The forward reaction is spontaneous. B. ?G° = 70 . 91

Question

A. ?G° = 141.8 kJ?/?mol. The forward reaction is spontaneous. B. ?G° = 70.91 kJ?/?mo.. The forward reaction is nonspontaneous. C. ?G° = 141.8 kJ?/?mol. The forward reaction is nonspontaneous. D. ?G° = 141.8 kJ?/?mol. The reaction is at equilibrium. Look at the following reaction. 2SO_3 (g) 2SO_2(g) + O_2 (g) Suppose that you are given the following information for this reaction at room temperature DeltaGdegree_f for O_2 (g) = 0. 0 kj/mol DeltaG^degree_f for SO_3 (g) = -371.1 kJ/mol Find the value for DeltaG degreee for this reaction and state whether the forward reaction is spontaneous, non spontaneous, or at equilibrium.

Explanation / Answer

Ans B is correct

Go of the reaction = Go product - Go reactant

= (-300.19 + 0) - (-371.1) kJ/mol

= 70.91 kJ/mol

Since Go is positive for forward reaction, the reaction is nonspontaneous

(note: So backward reaction will be spontaneous)

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