Electrolysis and Faraday's Law - AP Chemistry

The oxidation number increases at the anode. Oxidation involves loss of electrons, increasing oxidation state.

96500 coulombs is the charge of 1 mole of electrons. Faraday's constant relates charge to moles of electrons.

The anode typically dissolves into the solution. Active anodes oxidize and release metal ions into solution.

Larger surface area increases the rate of electrolysis. Greater area provides more sites for electron transfer reactions.

The standard reduction potential for Ag$^+$ is +0.80 V. Standard electrode potential for silver reduction reaction.

Hydrogen gas (H₂) is the main product. Water reduction produces hydrogen gas at the negative electrode.

The oxidation number increases at the anode. Oxidation involves loss of electrons, increasing oxidation state.

Larger surface area increases the rate of electrolysis. Greater area provides more sites for electron transfer reactions.

The rate of electrolysis is primarily affected by the current. Higher current drives more electrons through the circuit faster.

The unit of electric current is amperes (A). Standard unit for measuring electrical current flow.

Equivalent weight = $\frac{\text{Atomic weight}}{\text{Valence}}$. Atomic mass divided by oxidation state change in reaction.

The mass of substance liberated is proportional to the charge passed. More charge produces proportionally more product deposition.

96500 coulombs is the charge of 1 mole of electrons. Faraday's constant relates charge to moles of electrons.

Charge (C) = Current (A) $\times$ Time (s). Product of current and time gives total charge passed.

96500 coulombs are required. One Faraday deposits one equivalent of any substance.

An electrolyte is a substance that produces ions when dissolved in water, conducting electricity. Ionic compounds enable current flow in aqueous solutions.

Charge = $0.5 \times 2 \times 96500 = 96500$ C. Multiply moles by valence then by Faraday's constant.

The oxidation state decreases as the metal is reduced. Metal cations gain electrons, reducing their oxidation state.

Equivalent weight = $\frac{56}{2} = 28$ g/equiv. Divide atomic weight by the number of electrons transferred.

Inert electrodes conduct electricity without participating in the reaction. Unreactive electrodes only transfer electrons, don't dissolve.

Higher temperature increases the rate of electrolysis. Heat increases ion mobility and reaction kinetics.

Increases the efficiency and rate of electrolysis. More ions improve conductivity and reaction kinetics.

3 moles of electrons are needed. Aluminum has +3 charge, requiring 3 electrons for reduction.

An anode is the electrode where oxidation occurs. Positive electrode where electrons are lost from species.

The anode typically dissolves into the solution. Active anodes oxidize and release metal ions into solution.

A diaphragm separates the anode and cathode to prevent mixing of products. Physical barrier prevents product recombination and contamination.