3 posts • Page 1 of 1
Generally, a negative E° means the reaction is unfavorable. This is because in the equation ∆G°(redox)= -nFE°, a negative E° would yield a positive ∆G°. When ∆G° is positive, that means the reaction is not spontaneous and thereby unfavorable.
To determine if a redox reaction is favorable, you must first figure out the E° of the reaction. This is easiest done by splitting the overall reaction into its half-reactions. After determining which half-reaction is the oxidation reaction and which is the reduction reaction, find the respective standard potentials using the table in the book. Then apply the formula, E° = E°(cathode) - E° (anode) to determine the overall E°. If E° is greater than zero, the reaction is spontaneous/favorable (because K>1 and delta G<0). Hope this helps!
Who is online
Users browsing this forum: No registered users and 0 guests