Chapter 18 Flashcards
Non-Standard State Solutions
∆G = ∆Go + RTln(Q)
Electrochemical Cell
A device in which a chemical reaction either produces or is carried out by an electrical current.
Voltaic (Galvanic Cell)
An electrochemical cell that produces electrical current from a spontaneous chemical reaction.
Electrolytic Cell
Consumes electrical current to drive a nonspontaneous chemical reaction.
Half-Cell
One half of an electrochemical cell where either oxidation or reduction occurs.
Electrodes
Conductive surfaces through which electrons can enter or leave the half-cells.
Amperes (A)
- Measure of electrical current.
- 1 A = 1 C/s
Potential Difference
A measure of the difference in potential energy per unit of charge (J/C)
1 J/C = V
Electromotive Force (emf)
The force that results in the motion of electrons due to a difference in potential.
Cell Potential/Cell emf (Ecell)
The potential difference between the two electrodes (in a voltaic cell)
- Depends on:
- Depends on tendencies of reactants to undergo oxidation and reduction.
- Depends on the concentrations of the reactants and products in the cell.
- Temperature.
Standard Cell Potential / Standard emf (Eocell)
- I M concentration for reactants in solution
- 1 atm for pressure for gaseous reactants
- Temperature: 25oC
Anode
- Electrode where oxidation occurs.
- More negatively charged electrode.
Cathode
- Electrode where reduction occurs.
- More positivetly charged electrode.
Salt Bridge
- Inverted, U-shaped tube that contains a strong electrolyte such as KNO3 and connects the two half-cells.
- Allows a flow of ions that neutralize the charge buildup in the solution.
- The (-) ions within the salt bridge flow to neutralize the accumulation of postive charge at the anode, and the (+) ions flow to neutralize the accumulation of negative charge at the cathode (The salt bridge completes the circuit).
Cell Diagram / Line Notation
- Oxidation half-reaction written on the left.
- Reduction half-reaction written on the right.
- Substances in different phases are separated by a single vertical line.
- Reactant and products of one or both of the half-reactions may be in the same phase, where we then separate them from each other with a comma.
- A double vertical line (salt bridge) separates the two half-reactions.
Example:
Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s)
Standard Electrode Potential
The overall standard cell potential (Eocell) is the difference between the two stard electrode potentials.