Electrochemistry Practice Problems

These flashcards cover key vocabulary and concepts related to electrochemistry based on the provided lecture notes.

Oxidation

Involves a loss of electrons and occurs at the anode.

Reduction

Involves a gain of electrons and occurs at the cathode.

Anode

Electrode where oxidation occurs and electrons are lost.

Cathode

Electrode where reduction occurs and electrons are gained.

Salt Bridge

Used to maintain charge balance in electrochemical cells.

Galvanic Cell

A type of electrochemical cell that generates electrical energy from spontaneous chemical reactions.

Cell Potential

The voltage produced by an electrochemical cell, can be positive or zero, but never negative for galvanic cells.

Net Cell Potential

The overall voltage calculated from the standard reduction potentials of the half reactions.

Faraday's Constant

The electric charge carried by one mole of electrons, approximately 96485 coulombs.

Gibbs Free Energy (ΔG)

A thermodynamic potential that measures the useful work obtainable from a thermodynamic system.

Current (I)

The flow of electric charge, measured in amperes (A).

Charge (Q)

Total electric charge, calculated as current (I) multiplied by time (t).

Oxidation State

The hypothetical charge that an atom would have if all bonds were completely ionic.

Electroplating

The process of depositing a layer of metal onto a surface through electrolysis.

Standard Line Notation

A shorthand representation of an electrochemical cell showing the anode and cathode materials, phase changes, and concentrations.

Electrons flow from the…

anode to the cathode in an electrochemical cell.

Increase in product concentration

increases the voltage of the cell.

Increase in reactant concentration

decreases the voltage of the cell.

Relation Between K, Delta G, and Ecell