For a reaction with ${\mathbf{\Delta H}}^{\mathbf{°}}\mathbf{=}\mathbf{40}\mathbf{}\mathbf{kJ}\mathbf{/}\mathbf{mol}$, decide which of the following statements is (are) true. Correct any false statement to make it true. (a) ${\mathbf{\Delta G}}^{\mathbf{°}}$The reaction is exothermic; (b) for the reaction is positive; (c) ${\mathbf{K}}_{\mathbf{eq}}$ is greater than 1; (d) the bonds in the starting materials are stronger than the bonds in the product; and (e) the product is favored at equilibrium.

A negative value of ${\mathbf{\Delta H}}^{\mathbf{°}}$for a reaction indicates that the products are favored while a positive value indicates that reactants (i.e., the starting materials) are favored.

${\mathrm{\Delta H}}^{°}$is directly related to ${\mathrm{\Delta G}}^{°}$and hence, the negative value of ${\mathrm{\Delta G}}^{°}$ also indicates that the products are favored.

The correct statement should be - The reaction is endothermic.

True, since${\mathrm{\Delta H}}^{°}$is directly related to${\mathrm{\Delta G}}^{°}$, a positive value of${\mathrm{\Delta H}}^{°}$corresponds to a positive value of${\mathrm{\Delta G}}^{°}$.

False, as the positive value of${\mathrm{\Delta H}}^{°}$indicates that the reaction favors the reactants (i.e., the reaction proceeds backward).

The value of ${\mathrm{K}}_{\mathrm{eq}}$ for a backward reaction is always less than 1.

True, Positive value of ${\mathrm{\Delta H}}^{°}$ indicates that the reactants or the starting materials are stronger than the bonds in the product.

False, the reactants are favored at equilibrium as ${\mathrm{\Delta H}}^{°}$is positive.