If the delta G of the reaction A->B is -12.5 kJ/mol (-3.0 kcal/mol), which of th

ID: 174295 • Letter: I

Question

If the delta G of the reaction A->B is -12.5 kJ/mol (-3.0 kcal/mol), which of the following statements are correct? Pick all that apply

A. the reaction will proceed spontaneously from left to right at the given conditions

B. the reaction will proceed spontaneously from right to left at the given conditions

C. the equilibrium constant favors the formation of B over the formation of A

D. the equilibrium constant can be calculated if the initial concentrations of A and B are known

E. the value of delta G0' is also negative

Answer is A. the reaction will proceed spontaneously from left to right at the given conditions

D. the equilibrium constant can be calculated if the initial concentrations of A and B are known.

If Del G is negative, the reaction proceeds spontaneously to form products. (Forward)

If Del G is positive, the reaction proceeds spontaneously to form reactants. (Reverse)

If Del G is 0, the reaction is in equilibrium that is no further change in the concentration of reactants or products.

Equilibrium constant (K eq) is the ratio of concentration of products to reactants.

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