What is the difference between a spontaneous and non-spontaneous reaction in terms of Eยฐcell and ฮGยฐ?
Spontaneous: Eยฐcell > 0, ฮGยฐ < 0 | Non-spontaneous: Eยฐcell < 0, ฮGยฐ > 0
Compare and contrast oxidation and reduction.
Oxidation: Loss of electrons, occurs at the anode | Reduction: Gain of electrons, occurs at the cathode
What is the difference between standard cell potential and cell potential?
Standard cell potential is measured under standard conditions (1 M, 298 K, 1 atm), while cell potential is measured under non-standard conditions.
What is the effect of a positive Eยฐcell?
The reaction is spontaneous (thermodynamically favorable).
What is the effect of a negative Eยฐcell?
The reaction is non-spontaneous (thermodynamically unfavorable).
What happens to ฮGยฐ when Eยฐcell is positive?
ฮGยฐ becomes negative.
What happens to the equilibrium constant K, when ฮGยฐ is negative?
The equilibrium constant K, becomes greater than 1, indicating that products are favored at equilibrium.
What is the effect of increasing the concentration of reactants on cell potential?
According to Le Chatelier's principle, increasing reactant concentration generally increases the cell potential (shifts the equilibrium towards product formation).
What are the steps to calculate standard cell potential (Eยฐcell)?
1. Identify the cathode and anode. 2. Find the standard reduction potentials for the cathode and anode. 3. Apply the formula: Eยฐcell = Eยฐcathode - Eยฐanode.
Describe an alternative method to calculate Eยฐcell?
1. Reverse the oxidation half-reaction (change the sign of its potential). 2. Add the potentials of the reduction and oxidation half-reactions.
How do you calculate ฮGยฐ from Eยฐcell?
Use the formula: ฮGยฐ = -nFEยฐcell, where n is the number of moles of electrons transferred and F is Faraday's constant.
How do you calculate the equilibrium constant K, from ฮGยฐ?
Use the formula: $K = e^{\frac{-ฮGยฐ}{RT}}$ where R is the ideal gas constant and T is the temperature in Kelvin.
