Answer to Question #350669 in General Chemistry for Kell

Question

Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and Gibbs energy:

H = 8457J/mol,

S = 546J/K*mol, and

G = 432J at room temperature

Answer 1

A reaction with a negative value for ΔG releases free energy and is thus spontaneous. A reaction with a positive ΔG is nonspontaneous and will not favor the products.

∆G = 432 J is positive.

Answer: nonspontaneous