Answer:
Statements A and C are true.
Explanation:
<u>Let's evaluate the given statements:</u>
<u />
A) A reaction with negative Gibbs standard free energy (ΔG) will result in a reaction thermodynamically spontaneous, under standard conditions, by the Nernst equation:
(1)
<em>where n: is the number of electrons transferred in the cell reaction, F: is the Faraday constant and E: is the cell potential </em>
For an electrochemical reaction to be spontaneous, that is to say, in a galvanic cell, the change in Gibbs free energy must be negative. From equation (1), we have that a negative ΔG will result in a spontaneous electrochemical reaction.
Hence, statement A is correct, and D is incorrect.
C) A coupled redox reaction with a positive standard reduction potential is thermodynamically spontaneous:
On equation (1), for the Gibbs free energy to be negative and, therefore, the reaction to be thermodynamically spontaneous, the standard reduction potential must be positive.
Hence, statement C is correct, and B is incorrect.
I hope it helps you!