Electrode Potentials and Cell Reactions

The video tutorial by Ms. CM explains how to calculate cell potential using the standard electrode potential values. It covers the equation for cell potential, which is the difference between the reduction potential of the half-cell undergoing reduction and the half-cell undergoing oxidation. The tutorial provides examples using zinc-copper and magnesium-ion voltaic cells, demonstrating how to determine which half-cell undergoes oxidation or reduction based on their electrode potential values. The video emphasizes the importance of using standard reduction potentials as given in data booklets.

What is the formula used to calculate cell potential?

• E_red + E_ox

• E_red - E_ox

• E_ox + E_red

• E_ox - E_red

Which of the following is true about standard electrode potentials?

• They are intensive quantities.

• They are extensive quantities.

• They are multiplied by stoichiometric coefficients.

• They are always positive.

In a voltaic cell, which half cell undergoes oxidation?

• The one with a more positive electrode potential.

• The one with a more negative electrode potential.

• The one with zero electrode potential.

• The one with equal electrode potential.

For a zinc and copper voltaic cell, which half cell undergoes reduction?

• Both half cells

• Copper half cell

• Neither half cell

• Zinc half cell

What is the cell potential for a zinc and copper voltaic cell?

• 0.42 Volts

• 0.76 Volts

• 1.10 Volts

• 1.34 Volts

In a magnesium and iron voltaic cell, which half cell undergoes oxidation?

• Neither half cell

• Both half cells

• Iron half cell

• Magnesium half cell

What is the cell potential for a magnesium and iron voltaic cell?

• 1.10 Volts

• 2.37 Volts

• 0.45 Volts

• 1.92 Volts

Which half cell has a more negative reduction potential in a magnesium and iron voltaic cell?

• Neither has a negative potential

• Magnesium half cell

• Iron half cell

• Both have the same potential

What is the significance of a more positive electrode potential in a half cell?

• It indicates oxidation.

• It indicates reduction.

• It indicates no reaction.

• It indicates equilibrium.

How are standard electrode potentials used in calculations?

• They are subtracted from each other.

• They are divided by each other.

• They are added together.

• They are multiplied by stoichiometric coefficients.