Reaction 1 (A⟶B) has a ΔG=+3 kJ/mol, reaction 2 (B⟶C) has a ΔG=-6kJ/mol, and reaction 3 (C⟶D) has a ΔG∘=+1 kJ / mol. If all of these are occurring in the same reaction sample, which statement is false? If the reactions of A⟶D are rearranged, they become non spontaneous. For D⟶A, ΔG∘=+2kJ/mol. Reaction 2 is driving reactions 1 and 3 forward. A⟶D is thermodynamically spontaneous.

The statement 'If the reactions of A⟶D are rearranged, they become non spontaneous.' is false

Explanation:

Step 1: Data given

Reaction 1 (A⟶B) has a ΔG=+3 kJ/mol

Reaction 2 (B⟶C) has a ΔG=-6kJ/mol

Reaction 3 (C⟶D) has a ΔG=+1 kJ / mol.

Step 2:

To be spontaneous ΔG should be negative (ΔG<0)

For reaction A⟶D; ΔG = 3kJ/mol - 6kJ/mol + 1 kJ/mol = - 2 kJ/mol

This means for the reaction A⟶D; the reaction is spontaneous

This means for the reaction D⟶A; ΔG = 2kJ/mol, so the reaction is non-spontaneous

For reaction 1 and 3 the reaction is, non-spontaneous (but the reverse reaction is). Reaction 2 is driving reactions 1 and 3 forward. A⟶D is thermodynamically spontaneous.

The statement 'If the reactions of A⟶D are rearranged, they become non spontaneous.' is false