Applications of Thermodynamics

Applying a higher current through the circuit.

Decreasing ambient light during electrolysis.

Altering electrode shape without changing surface area.

Using a longer electrolyte bridge between electrodes.

E = E_reduction * E_oxidation

E = E_reduction + E_oxidation

E = E_reduction - E_oxidation

E = E_oxidation - E_reduction

Galvanic cells convert electrical energy into chemical energy.

Galvanic cells can operate without an external source of electrical energy.

Galvanic cells convert chemical energy into electrical energy.

Galvanic cells require an external source of electrical energy to operate.

Reduction potential for both metals decreases as increased thermal motion disrupts electron uptake ability at each electrode surface.

Both Ag and Ni experience an increase in their reduction potentials with rising temperatures due to increased kinetic energy of ions.

No effect because standard reduction potentials are defined at standard conditions including temperature.

Temperature increase lowers Ag's reduction potential but increases Ni’s due to differing activation energies.

Neither electrode changes in mass.

Both electrodes equally increase in mass.

Anode.

Cathode.

n = F^(2)/Q

n = F / Q

n = Q * F

n = Q / F

Ecell_ = Eanode - Ecathode

Ecell = Eanode * Ecathode

Ecell = Ecathode - Eanode

Ecell = Ecathode + Eanode

The electrode potential would decrease since increasing pressure would always oppose reaction progress regardless of whether gases are involved or not at one electrode's compartment.

The electrode potential may increase if gas is involved and pressure is increased at that electrode's compartment according to Le Chatelier’s principle.

Pressure changes do not impact E because it only depends on concentrations of aqueous solutions, not gases at one electrode's compartment.

Changing pressure has negligible effects since solids' activities are constants, so any change won't significantly impact E at one electrode's compartment even with gases present.

amperes

volts

Newtons

ohms

Reduction reaction.

Oxidation reaction.

Deposition of metal ions.

Salt bridge formation.