All Flashcards
Define E°cell.
Cell potential under standard conditions (298.15 K, 1 atm, 1 M concentrations).
Define Ecell.
Cell potential under non-standard conditions.
Define the reaction quotient, Q.
A measure of the relative amount of products and reactants present in a reaction at a given time. Used to determine if a reaction is at equilibrium.
Define Faraday's constant (F).
The charge of one mole of electrons, approximately 96485 C/mol e-.
Define 'n' in the Nernst Equation.
Moles of electrons transferred in the balanced redox reaction.
Differentiate between E°cell and Ecell.
E°cell: Cell potential at standard conditions. | Ecell: Cell potential at non-standard conditions.
Compare the conditions when Q = 1 versus Q ≠ 1.
Q = 1: Standard conditions, all concentrations are 1 M. | Q ≠ 1: Non-standard conditions, concentrations are not 1 M.
How does Q relate to K at equilibrium and non-equilibrium?
At equilibrium: Q = K. | Non-equilibrium: Q ≠ K.
What is the difference between a voltaic cell at equilibrium and non-equilibrium?
Non-equilibrium: Running galvanic cell, Ecell > 0. | Equilibrium: Dead battery, Ecell = 0.
Compare the effect of Q > 1 and Q < 1 on Ecell.
Q > 1: Ecell < E°cell. | Q < 1: Ecell > E°cell.
What is the effect of increasing product concentration on Q?
Q increases.
What is the effect of Q > 1 on Ecell?
Ecell decreases (Ecell < E°cell).
What happens to Ecell as a galvanic cell approaches equilibrium?
Ecell decreases and approaches 0.
What happens to ΔG when Ecell is positive?
ΔG is negative, indicating a spontaneous reaction.
What is the impact of increasing the concentration of reactants on the cell voltage?
The cell voltage increases.