Biochemical Cell Potentials: Example 1

The video tutorial explains the concept of cell potentials in oxidation-reduction reactions and demonstrates how to calculate the cell potential, standard Gibbs free energy, and equilibrium constant for a given reaction. It covers the reduction and oxidation processes, the use of the Faraday constant, and the application of thermodynamic equations to derive these values.

What is the primary purpose of calculating cell potentials in oxidation-reduction reactions?

• To measure the temperature change

• To calculate Gibbs free energy and equilibrium constants

• To find the reaction rate

• To determine the color change in reactions

Which of the following is a reduction reaction?

• Acetaldehyde to Ethanol

• FADH2 to FAD

• NAD to NADH

• NADH to NAD

How is the oxidation potential for ethanol to acetaldehyde determined?

• By using the reduction potential directly

• By flipping the sign of the reduction potential

• By adding the reduction potential

• By multiplying the reduction potential by two

What is the Faraday constant used in calculating the standard free energy change?

• 2 electrons

• 8.314 J/mol K

• 96,485 J/mol V

• 0.123 V

How many electrons are transferred in the reaction involving NAD and ethanol?

• Four electrons

• Three electrons

• Two electrons

• One electron

What is the relationship between standard free energy change and the equilibrium constant?

• Directly proportional

• Inversely proportional

• No relationship

• Exponentially related

What is the equilibrium constant for the reaction at 300 Kelvin?

• 0.736

• 7.36

• 7.36 x 10^-5

• 7.36 x 10^5