Electrochemistry Basics

What is electrode potential?

• Electrode potential is the measure of the amount of water in an electrolyte

• Electrode potential is the measure of the color change in an electrolyte

• Electrode potential is the measure of the temperature of an electrolyte

• Electrode potential is the measure of the tendency of an electrode to lose or gain electrons when it is in contact with an electrolyte.

Define standard electrode potential.

• Standard electrode potential is the measure of the tendency of a half-cell to form covalent bonds.

• Standard electrode potential is the measure of the tendency of a half-cell to gain electrons and be oxidized.

• Standard electrode potential is the measure of the tendency of a half-cell to attract protons.

• Standard electrode potential is the measure of the tendency of a half-cell to lose electrons and be reduced.

State the Nernst equation.

• Ecell = E°cell - (RT/nF) * ln(Q)

• Ecell = E°cell + (RT/nF) * ln(Q)

• Ecell = E°cell - (RT/nF) * log(Q)

• Ecell = E°cell - (RT/nF) * ln(K)

How is cell potential calculated?

• Ecell = Ecathode + Eanode

• Ecell = Ecathode x Eanode

• Ecell = Ecathode / Eanode

• Ecell = Ecathode - Eanode

What is the unit of electrode potential?

• newtons (N)

• joules (J)

• volts (V)

• amperes (A)

Explain the significance of standard hydrogen electrode.

• The significance of the standard hydrogen electrode lies in its role as a reference point for measuring electrode potentials.

• The standard hydrogen electrode is primarily used in organic chemistry experiments.

• It is a tool for measuring temperature in chemical reactions.

• The standard hydrogen electrode is used for electrolysis in batteries.

How does temperature affect the Nernst equation?

• Temperature affects the Nernst equation by changing the number of electrons transferred

• Temperature affects the Nernst equation by modifying the electrode potential

• Temperature affects the Nernst equation by altering the concentration of reactants

• Temperature affects the Nernst equation by changing the value of the gas constant (R) and the Faraday constant (F).

Calculate the cell potential when E°cell = 1.23 V and Q = 0.001.

• 1.230 V

• 1.220 V

• 1.234 V

• 1.4076 V

Determine the standard electrode potential for the reaction Zn(s) + Cu2+(aq) -> Zn2+(aq) + Cu(s).

• +0.34 V

• -0.76 V

• +1.44 V

• -1.98 V

If the concentration of Cu2+ ions is 0.1 M and Cu(s) is at 1 atm, calculate the cell potential for the given reaction.

• 0.25 V

• 0.42 V

• 0.18 V

• 0.34 V