Nernst Equation and Cell Potential

The video tutorial explains how to determine the electrode potential or EMF of a cell, focusing on the oxidation of tin and reduction of lead. It covers the concepts of anode and cathode, standard electrode potentials, and the calculation of cell potential using the Nernst equation. The tutorial also discusses the reaction quotient Q and its role in determining cell potential under non-standard conditions.

What happens to tin in the oxidation-reduction process described?

• It remains unchanged.

• It loses two electrons.

• It gains two electrons.

• It gains one electron.

In the standard electrode potential table, how are reactions typically written?

• As reduction reactions.

• As spontaneous reactions.

• As neutral reactions.

• As oxidation reactions.

Which electrode is always on the left in the cell notation?

• Neither

• Anode

• Cathode

• Both

How is the standard EMF of a cell calculated?

• By adding the potentials of the anode and cathode.

• By subtracting the anode potential from the cathode potential.

• By multiplying the potentials of the anode and cathode.

• By dividing the cathode potential by the anode potential.

What is the standard EMF of the cell if all concentrations are 1.0 molar?

• 0.001 volts

• 1.0 volts

• 0.01 volts

• 0.1 volts

What does the Nernst equation help calculate?

• The standard EMF of a cell.

• The cell potential under non-standard conditions.

• The concentration of reactants.

• The equilibrium constant.

What is the correction factor in the Nernst equation?

• 0.0592 divided by the number of electrons exchanged.

• 0.0592 multiplied by the number of electrons exchanged.

• 0.0592 added to the number of electrons exchanged.

• 0.0592 subtracted from the number of electrons exchanged.

What is the value of Q in the Nernst equation for this reaction?

• 1000

• 10

• 1

• 0.1

What is the final calculated cell potential using the Nernst equation?

• -0.0788 volts

• 0.0788 volts

• 0.01 volts

• -0.01 volts

Why is the cell reaction not spontaneous?

• Because the cell potential is negative.

• Because the concentration of reactants is too high.

• Because the cell potential is positive.

• Because the concentration of products is too high.