AP Chemistry Flashcards: Cell Potential Under Nonstandard Conditions
Written by AP Content Team, Verified for 2026 AP Exams, Last updated: May 2026
Review key ideas with interactive flashcards. This set includes 10 cards to help you master important concepts.
According to Le Châtelier's principle, what happens to the cell potential (E) if the concentration of a product is increased above standard conditions?
Increasing the concentration of a product will shift the reaction in reverse, decreasing the driving force and thus decreasing the cell potential (E < E°).
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According to Le Châtelier's principle, what happens to the cell potential (E) if the concentration of a product is increased above standard conditions?
Increasing the concentration of a product will shift the reaction in reverse, decreasing the driving force and thus decreasing the cell potential (E < E°).
What is the fundamental purpose of the cell potential in a reaction?
The cell potential serves as the driving force that moves a reaction toward a state of equilibrium.
What does the term 'Q' represent in the Nernst equation?
The term 'Q' represents the reaction quotient, which accounts for the current concentrations of products and reactants under nonstandard conditions.
What is the Nernst equation?
The Nernst equation ($$E = E^\circ - \frac{RT}{nF} \ln Q$$) is the formula that describes how cell potential (E) varies with species concentrations under nonstandard conditions.
What are nonstandard conditions in the context of electrochemical cells?
Nonstandard conditions refer to any state where the concentrations of the species involved in the cell reaction are not at the standard state (typically 1 M for solutes).
For the AP exam, what principle is typically used to qualitatively assess changes in cell potential under nonstandard conditions?
Le Châtelier's principle is often used to qualitatively determine how changes in concentration will shift the reaction and affect the overall cell potential.
What does a large magnitude for cell potential (E) signify?
A large magnitude for the cell potential signifies a large driving force, indicating that the reaction is far from equilibrium.
How do deviations from standard conditions affect cell potential?
Deviations from standard conditions, specifically changes in species concentrations, cause the cell potential to vary from the standard cell potential (E°).
What is the relationship between a cell's potential and its proximity to equilibrium?
The cell potential drives the reaction toward equilibrium. The farther the system is from equilibrium, the greater the magnitude of the cell potential.
According to Le Châtelier's principle, what happens to the cell potential (E) if the concentration of a reactant is increased above standard conditions?
Increasing the concentration of a reactant will shift the reaction forward, increasing the driving force and thus increasing the cell potential (E > E°).