Electrochemistry Formulas & Things to Remember

Faraday’s Constant

96485 C/mol

A (ampere)

1 C/sec

Volt (V)

1 J/C

C

coulumb

What is EMF

volts (Joules or work / Coulumb or charge)

In a voltaic cell, electrons travel from

anode to cathode

Anodes are

oxidized

Cathodes are

reduced

Any species of a half-reaction will be spontaneous with a reverse half-reaction ___ the first one on the table

below

E⁰

w / q

w =

-q * E⁰

W_^max

-q * E⁰

W_max also equals

-nFE⁰

Change in G⁰

-nFE⁰_cell = -RTlnK

Nernst Equation

E_cell = E⁰ - 0.0592/N * logQ

E⁰ equals (from Nernst equation)

.0592/N * logQ

Electrolytic Cell

nonspontaneous = uses electrical energy from external source to make another nonspontaneous reaction

Cathode charge in galvanic cell

+

Anode charge in galvanic cell

-

Cathode charge in electrolytic solution

-

Anode charge in electrolytic solution

+

Faraday’s law

the amount of substance to be oxidized or reduced at each electrode during electrolysis is directly proportional to the amount of electricity that pass through the cell