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.

Galvanic cells use salt bridges to maintain neutrality while electrolytic cells do not use salt bridges as components.

Galvanic cells use spontaneous redox reactions to generate electricity while electrolytic cells require an external power source.

Galvanic cells produce gases during operation while electrolytic cells do not produce gases as byproducts of their chemical reactions.

Electrolytic cells are able to operate under standard conditions while galvanic cells cannot operate without being charged first.

A fuel cell used to generate electricity in a car.

A battery powering a flashlight.

An electroplating cell used to deposit a metal coating onto a surface.

A galvanic cell used to power a calculator.

Use wires with lower electrical resistivity for connections

Switching from an acidic electrolyte to one that is more basic if it results in lower ionization energy metals present as reactants

Increase surface area of electrodes without changing their material

Increase concentration of reactant ions within one-half cell only

Decreasing the distance between electrodes within each cell.

Connecting multiple cells in series.

Ensuring high concentrations of electrolyte solutions.

Using more reactive metals for electrodes.

Ecell_ = Eanode - Ecathode

Ecell = Eanode * Ecathode

Ecell = Ecathode - Eanode

Ecell = Ecathode + Eanode

Decreases voltage due to lower reduction potential at cathode.

Increases voltage due to higher reduction potential at cathode.

Increases voltage due to higher oxidation potential at anode.

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.

E = E_reduction * E_oxidation

E = E_reduction + E_oxidation

E = E_reduction - E_oxidation

E = E_oxidation - E_reduction

amperes

volts

Newtons

ohms