Sab Electrochemistry Nernst Equation

Write the half-cell reaction for the reduction of Cu2+ to Cu.

• Cu2+ + e- -> Cu

• Cu2+ + 2e- -> Cu

• Cu2+ -> Cu + 2e-

• Cu2+ + 3e- -> Cu

Derive the Nernst equation for a galvanic cell.

• Ecell = E°cell - (RT/nF) * log(Q)

• Ecell = E°cell + (RT/nF) * ln(Q)

• Ecell = E°cell + (RT/nF) * log(Q)

• Ecell = E°cell - (RT/nF) * ln(Q)

What is the standard electrode potential of the hydrogen electrode?

• 0 V

• -1 V

• 1 V

• 2 V

Calculate the cell potential for the reaction: Zn(s) + Cu2+(aq) -> Zn2+(aq) + Cu(s) given E°cell = 1.10 V.

• 1.10 V

• 0.90 V

• 1.50 V

• 1.01 V

Explain the concept of concentration cells and provide an example.

• Concentration cells do not rely on differences in ion concentration to generate electricity

• A concentration cell involves the use of a single type of electrode

• An example of a concentration cell is a battery with two different metals as electrodes

• An example of a concentration cell is two half-cells with silver electrodes immersed in solutions of different concentrations of silver nitrate. The cell generates electricity as silver ions move from the higher concentration side to the lower concentration side.

Identify the half-cell reaction for the oxidation of Fe2+ to Fe3+.

• Fe3+ -> Fe2+ + e-

• Fe2+ + 2e- -> Fe3+

• Fe2+ + e- -> Fe3+

• Fe2+ -> Fe3+ + e-

How does temperature affect the Nernst equation?

• Temperature affects the Nernst equation by altering the speed of light constant.

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

• Temperature affects the Nernst equation by modifying the value of Planck's constant.

• Temperature affects the Nernst equation by changing the value of Avogadro's number.

What is the standard electrode potential of the standard hydrogen electrode?

• 1 V

• 2 V

• -1 V

• 0 V

Determine the cell potential for the reaction: Pb(s) + 2Ag+(aq) -> Pb2+(aq) + 2Ag(s) with E°cell = 0.46 V.

• 0.25 V

• 0.52 V

• 0.34 V

• 0.40 V

Discuss the applications of concentration cells in electrochemistry.

• Concentration cells are used to generate electricity from chemical reactions

• Concentration cells are primarily used in agriculture for soil testing

• Concentration cells are applied in electrochemistry to measure temperature changes

• Concentration cells are applied in electrochemistry to measure ion concentrations in solutions and study the impact of concentration gradients on cell potential.