Electrochemistry Concepts Quiz

Standard Electrode Potential (Eo)

• The standard electrode potential (Eo) is a measure of the tendency of a metal to lose electrons and get oxidized.
• The greater the negative value of the Eo, the greater the tendency of the metal to form its ionic state.
• The standard electrode potential is also a measure of the reducing strength of the metal.
• The standard hydrogen electrode (NHE) has a potential of zero.

Solution Pressure (S.P.) and Ionic Pressure (I.P.)

• Solution Pressure is the tendency of a metal to dissolve and form cations.
• Ionic Pressure is the tendency of metal cations in a solution to be deposited on the metal rod.
• The predominant process depends on the nature of the metal and the concentration of the solution.

Half-Cell and Single Electrode Potential

• A half-cell consists of a metal rod immersed in a solution of its ions.
• The potential difference between the metal rod and its solution is called the single electrode potential.
• The sign of the potential is the same as the charge on the metal electrode.
• The single electrode potential is a measure of the tendency of the metal to be oxidized or reduced.

Galvanic Cell or Voltaic Cell

• When two half-cells are connected, electrons pass from the half-cell with a higher tendency to oxidize to the half-cell with a higher tendency to reduce.
• This flow of electrons creates an electric current in the cell.
• The potential difference between the two half-cells is called the electromotive force (emf) of the cell.

Redox Reactions

• Oxidation is the loss of electrons.
• Reduction is the gain of electrons.
• Oxidants (oxidizing agents) are electron acceptors.
• Reductants (reducing agents) are electron donors.
• Redox reactions involve the transfer of electrons from a reductant to an oxidant.
• Each redox reaction can be represented by two half-reactions: one for oxidation and one for reduction.

Half-Reactions of Oxidants and Reductants

• Half-reactions of Oxidants:

  • MnO4- + 8H+ + 5e- = Mn2+ + 4H2O
  • Ce4+ + e- = Ce3+
  • Cr2O72- + 14H+ + 6e- = 2Cr3+ + 7H2O
  • I2 + 2e- = 2I-

• Half-reactions of Reductants:

  • C2O42- = 2CO2 + 2e-
  • 2I- = I2 + 2e-
  • 2S2O32- = S4O62- + 2e-
  • NO2- + H2O = NO3- + 2H+ + 2e-

Test your knowledge on standard electrode potential, solution pressure, and ionic pressure. This quiz covers key definitions and principles related to half-cell and single electrode potential. Challenge yourself and enhance your understanding of electrochemistry.