All Flashcards
Define 'thermodynamically favorable reaction'.
A reaction that occurs spontaneously, with ΔG° < 0 and K > 1.
Define 'thermodynamically unfavorable reaction'.
A reaction that does not occur spontaneously, with ΔG° > 0 and K < 1.
Define 'electrolytic cell'.
A cell that uses electrical energy to drive a nonspontaneous redox reaction.
Define 'coupled reactions'.
Reactions that involve a nonspontaneous reaction and a spontaneous reaction that share a common intermediate, allowing the nonspontaneous reaction to proceed.
Define 'common intermediate'.
A substance produced in one step of a reaction mechanism and consumed in a later step.
What is the effect of a positive ΔG° on a reaction's spontaneity?
The reaction is nonspontaneous and requires an external energy source to proceed.
What is the effect of coupling a nonspontaneous reaction with a highly spontaneous reaction?
If the spontaneous reaction's negative ΔG° is large enough, the overall coupled reaction becomes spontaneous.
What is the effect of multiplying a reaction by a coefficient on its ΔG° value?
The ΔG° value is multiplied by the same coefficient.
What is the effect of adding two reactions together?
The ΔG° values of the two reactions are also added together to find the ΔG° of the overall reaction.
What is the effect of using an external power source on a nonspontaneous reaction in an electrolytic cell?
The external power source provides the necessary energy to drive the nonspontaneous reaction forward.
What are the key differences between thermodynamically favorable and unfavorable reactions?
Favorable: ΔG° < 0, K > 1, spontaneous | Unfavorable: ΔG° > 0, K < 1, nonspontaneous.
What are the differences between voltaic and electrolytic cells?
Voltaic: Spontaneous redox reaction, produces electricity | Electrolytic: Nonspontaneous redox reaction, requires electricity.