A reaction where both reactants get reduced.

A reaction where both reactants get oxidized.

A reaction that involves a transfer of electrons between reactants.

A reaction that involves the combustion of at least one reactant.

It is a cell that destroys electrons on one side and creates electrons on the other side.

It is a cell that contains only one metal bar and one aqueous ion solution.

It is a type of battery that generates an electrical current from redox reactions.

It is a type of battery that drives a redox reaction when electricity is applied.

It converts chemical energy into electrical energy

To set up this cell, a salt bridge is used

The reactions taking place are non-spontaneous

The electrolytes taken in the two beakers are different

Cu

ZnSO4

CuSO4

Zn

is not necessary in order for the cell to work

allows charge balance to be maintained in the cell

drives free electrons from one half-cell to the other

is tightly plugged with firm agar gel through which ions cannot pass

a phase boundary

gas electrode

a wire (metal) connection

a salt bridge

Sn⁴⁺

Sn²⁺

Fe³⁺

Fe²⁺

Ni²⁺ + 2e^- → Ni

Ag⁺ + e^- →Ag

Ag → Ag⁺ + e^-

Ni → Ni²⁺ + 2e^-

is called the cathode

is oxidized

gains mass at the electrode

decreases in oxidation number

chemical reaction

physical reaction

no reaction

none of above

mechanical energy in to electrical energy

potential energy in to electrical energy

electrical energy in to chemical energy

chemical energy in to electrical energy

completes the circuit so that electrons can flow through the wire

maintains electrical neutrality

avoid liquid junction potential

all of the above

the metal to be plated

ions of the plating metal

any type of metal

no metal ions

Anode: Pb²⁺, Cathode: Cu

Anode: Pb, Cathode: Cu

Anode: Pb, Cathode: Cu²⁺

Anode: Pb, Cathode: Cu²⁺

E_cell = E⁰_cell - $$\frac{RT}{nF}$$  ln $$\frac{\left[Al^{3+}\right]^2}{\left[H^+\right]^6}$$  

E_cell = E⁰_cell - $$\frac{RT}{nF}$$  ln $$\frac{\left[H^+\right]^6}{\left[Al^{3+}\right]^2}$$  

E_cell = E⁰_cell - $$\frac{RT}{nF}$$  ln $$\frac{\left[H^+\right]^6}{\left[Al^{3+}\right]^2\ \left(P_{H_2}\right)^3}$$  

E_cell = E⁰_cell - $$\frac{RT}{nF}$$  ln $$\frac{\left[Al^{3+}\right]^2\ \ \left(P_{H_2}\right)^3}{\left[H^+\right]^6}$$  

voltage provided

concentration of electrolyte

quantity of electricity passed

temperature of solution