Redox Reactions and Thermodynamics

The video tutorial explains the relationship between free energy and redox potential using the equation delta G = -nFE. It covers how to calculate delta G and the equilibrium constant K from the standard potential E. An example redox reaction is used to demonstrate these calculations, showing that a positive standard potential leads to a thermodynamically favored reaction with a negative delta G and a large equilibrium constant. The tutorial concludes with a summary of the implications of positive and negative standard potentials on reaction favorability and equilibrium.

What does the variable 'n' represent in the equation ΔG = -nFE?

• The number of moles of reactants

• The number of electrons transferred

• The temperature in Kelvin

• The potential of the reaction

How is ΔG° related to the equilibrium constant K?

• ΔG° is unrelated to K

• ΔG° is equal to K

• ΔG° is inversely proportional to K

• ΔG° is directly proportional to K

In the example redox reaction, what is the standard potential E°?

• 3.00 volts

• 2.00 volts

• 1.54 volts

• 0.00 volts

What is the value of ΔG° for the example redox reaction at 25°C?

• -446 kJ/mol

• 446 kJ/mol

• 100 kJ/mol

• 0 kJ/mol

What does a positive standard potential indicate about a reaction?

• The reaction does not occur

• The reaction is thermodynamically favored

• The reaction is at equilibrium

• The reaction is thermodynamically unfavorable

What happens to the equilibrium constant K when ΔG° is negative?

• K is equal to one

• K is greater than one

• K is less than one

• K is zero

If the standard potential E° is negative, what can be said about ΔG°?

• ΔG° is negative

• ΔG° is zero

• ΔG° is positive

• ΔG° is undefined

What does a positive ΔG° imply about the forward reaction?

• The reaction is at equilibrium

• The reaction is thermodynamically unfavorable

• The reaction is spontaneous

• The reaction is thermodynamically favored

When the equilibrium constant K is less than one, what does it indicate?

• No reaction occurs

• More reactants than products at equilibrium

• More products than reactants at equilibrium

• Equal amounts of reactants and products

What is the relationship between E° and ΔG° when E° is less than zero?

• E° is negative and ΔG° is positive

• E° is positive and ΔG° is negative

• E° and ΔG° are both positive

• E° and ΔG° are both negative