For a reaction with ΔH o = 65 kJ/mol, decide if the following statement is true. If the statement is false, choose the statement that makes it true. Select the single best answer.

The product is favored at equilibrium. (Assume the entropy term is small compared to the enthalpy term)

(A) The statement is false. The starting material is favored at equilibrium.

(B) The statement is true.

(C) The statement is false. Neither the product nor the starting material is favored at equilibrium.

(D) The statement is false. The equilibrium position of the reaction cannot be approximated

(A) The statement is false. The starting material is favored at equilibrium

Explanation:

As we know that type of reaction is predicted by value Gibbs free energy.

ΔG >0 It means that reaction is non spontaneous and favors the reactant of the reaction.

ΔG <0 It means that reaction is spontaneous and favors the product of the reaction.

As we know that

ΔG = ΔH - T ΔS

Here given that Assume the entropy term is small compared to the enthalpy term so ΔS = 0

⇒ ΔG = ΔH

Given that

ΔH o = 65 kJ/mol,

ΔG = ΔH = 65 kJ/mol

ΔG >0 It means that reaction is non spontaneous and favors the reactant of the reaction.

So the option A is correct.

(A) The statement is false. The starting material is favored at equilibrium.