Understanding the Nernst Equation

The video tutorial explains how to calculate cell potential using the Nernst equation, both in standard and non-standard states. It covers the components of the Nernst equation, such as the ideal gas constant, temperature, number of electrons, Faraday's constant, and reaction quotient. The tutorial uses a zinc-copper cell as an example to demonstrate how changes in ion concentration affect the instantaneous cell potential. It also discusses the relationship between cell potential, reaction progress, and equilibrium, highlighting how the Nernst equation predicts changes in cell potential as the reaction proceeds.

What is the term used for the cell potential at a specific moment in time?

• Equilibrium potential

• Reaction potential

• Standard cell potential

• Instantaneous cell potential

Which constant is NOT part of the Nernst equation?

• Temperature

• Boltzmann constant

• Ideal gas constant

• Faraday's constant

In the simplified Nernst equation, what is the value of the constant used when the temperature is 25 degrees Celsius?

• 0.0257 volts

• 0.0105 volts

• 0.1000 volts

• 0.0592 volts

For a zinc-copper cell, what is the standard cell potential at 25 degrees Celsius?

• 1.50 volts

• 1.10 volts

• 0.85 volts

• 0.75 volts

When the concentration of copper ions is 10.0 molar and zinc ions is 1.0 molar, how does the instantaneous cell potential compare to the standard cell potential?

• It is zero

• It is less than the standard cell potential

• It is equal to the standard cell potential

• It is greater than the standard cell potential

What happens to the instantaneous cell potential as the reaction progresses and the reaction quotient increases?

• It increases

• It decreases

• It remains constant

• It becomes zero

What is the relationship between delta G and the instantaneous cell potential when the reaction is thermodynamically favored?

• Delta G is positive

• Delta G is zero

• Delta G is undefined

• Delta G is negative

At equilibrium, what is the value of the instantaneous cell potential?

• Equal to the standard cell potential

• Zero

• Greater than the standard cell potential

• Less than the standard cell potential

When the reaction quotient Q equals the equilibrium constant K, what is the state of the reaction?

• The reaction is spontaneous

• The reaction is non-spontaneous

• The reaction is not at equilibrium

• The reaction is at equilibrium

According to the Nernst equation, when Q is less than 1, how does the instantaneous cell potential compare to the standard cell potential?

• It is zero

• It is greater than the standard cell potential

• It is equal to the standard cell potential

• It is less than the standard cell potential