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

i think it is true since you can test the answer and can use observations to complete it.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.