PCAT Chemical Processes – Standard Free Energy
- Oct 25, 2017
- PCAT Question of the Day
Which of the following statements most accurately describes the cell potential (Eo), change in Gibb’s free energy (ΔGo), and equilibrium constant (K) for a non-spontaneous chemical reaction?
- Eo < 0, ΔGo > 0, K < 1
- Eo < 0, ΔGo < 0, K < 1
- Eo > 0, ΔGo < 0, K > 1
- Eo > 0, ΔGo > 0, K > 1
This question is testing your understanding of the relationship between the change in standard free energy (ΔGo), electrochemical cell potential (Eo), and the equilibrium constant (K) for chemical reactions. To answer this question, you must apply the chemical principles relating to the equation, ΔG = -nFEcell, and a derivative of the Nernst Equation, ΔG = ΔGo + RTln(Q).
The question stem indicates that the chemical reaction is non-spontaneous, which corresponds to a positive change in standard free energy. According to the relationship between ΔGo and Eo based on the equation ΔGo = -nFEo, a positive ΔGocorresponds to a negative Eo. Thus, answer choices B and C can be eliminated. To determine the equilibrium constant, it is necessary to understand that the change in free energy of a chemical reaction (ΔG) is equal to zero and the reactant quotient (Q) is equal to the equilibrium constant (K). Thus, ΔGo = -RTln(K). Since ΔGo > 0, K < 1 making A the correct answer.
Search the Blog
Free ConsultationSchedule Now
MCAT Blog How to Review MCAT Full-Lengths
Free MCAT Practice AccountNeed great MCAT practice?
Get the most representative MCAT practice possible when you sign up for our free MCAT Account, which includes a half-length diagnostic exam and one of our full-length MCAT practice exams.Learn More