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What is the effect of increasing product concentration on Q?
Q increases.
What is the effect of Q > 1 on E<sub>cell</sub>?
E<sub>cell</sub> decreases (E<sub>cell</sub> < E°<sub>cell</sub>).
What happens to E<sub>cell</sub> as a galvanic cell approaches equilibrium?
E<sub>cell</sub> decreases and approaches 0.
What happens to ΔG when E<sub>cell</sub> 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.
Define E°<sub>cell</sub>.
Cell potential under standard conditions (298.15 K, 1 atm, 1 M concentrations).
Define E<sub>cell</sub>.
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.
How to determine Q for the reaction: $2Al(s) + 3Mn^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Mn(s)$?
Q = $\frac{[Al^{3+}]^2}{[Mn^{2+}]^3}$
Steps to predict E<sub>cell</sub> relative to E°<sub>cell</sub> using Q.
1. Calculate Q. 2. If Q > 1, E<sub>cell</sub> < E°<sub>cell</sub>. 3. If Q < 1, E<sub>cell</sub> > E°<sub>cell</sub>.
How do you calculate E°<sub>cell</sub> at equilibrium using the Nernst Equation?
Set E<sub>cell</sub> = 0 and Q = K in the Nernst Equation, then solve for E°<sub>cell</sub>.
What is the formula of Nernst Equation?
$E_{cell} = E^circ_{cell} - \frac{RT}{nF}lnQ$ or $E_{cell} = E^circ_{cell} - \frac{0.0592}{n}logQ$
How to relate ΔG to E<sub>cell</sub>?
ΔG = -nFE<sub>cell</sub>