#Non-Standard Conditions & Electrochemical Cells 🔋

Hey there, future AP Chem master! Let's dive into the world of electrochemical cells outside of standard conditions. It's all about how concentration, cell potential, and equilibrium play together. Get ready to make some awesome predictions!

#Comparing E_cell and E°_cell

Remember, standard conditions are 298.15 K, 1 atm, and 1 M concentrations (Q = 1). But what happens when we're not at these perfect conditions? That's where things get interesting!

• E°_cell is the cell potential under standard conditions.
• E_cell is the cell potential under non-standard conditions.

#The Nernst Equation

The Nernst Equation is our go-to tool for understanding how non-standard conditions affect cell potential. It relates E_cell to E°_cell and the reaction quotient, Q.

$$E_{cell} = E^\circ_{cell} - \frac{RT}{nF}lnQ$$

$$E_{cell} = E^\circ_{cell} - \frac{0.0592}{n}logQ$$

• R = 8.314 J/mol·K (gas constant)
• T = Temperature in Kelvin
• n = moles of electrons transferred in the balanced redox reaction
• F = Faraday's constant (96485 C/mol e-)

#Concentration and Cell Potential

Concentration is a major player in determining cell potential under non-standard conditions. Remember that:

$$Q = \frac{[Products]^n}{[Reactants]^m}$$

where n and m are the stoichiometric coefficients from the balanced reaction.

• If Q > 1 (too many products), E_cell < E°_cell...