We are being asked to determine which change will result to increase the voltage of the cell:
Al(s) | Al3+(aq, 1.00 M) || Cu2+(aq,1.00 M) | Cu(s)
In the Nernst Equation, we will calculate for Q where Q is equal to [products]/[reactants].
The Nernst Equation at 25°C:
Rewrite the Nernst Equation:
Ecell = cell potential under non-standard conditions
E°cell = standard cell potential
n = number of e- transferred
Q= reaction quotient = [products]/[reactants]
We have to write the overall reaction and determine the products and reactants:
Which of the following changes will increase the voltage of the cell Al(s)|Al3+(aq, 1.00 M)||Cu2+(aq,1.00 M)|Cu(s)?
I. Increasing the surface area of the Al electrode
II. Decreasing the concentration of Al3+(aq) to 0.001 M
III. Decreasing the concentration of Cu2+(aq) to 0.001 M
a. I and II`
b. I and III
c. I only
d. II only
e. III only
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the The Nernst Equation concept. You can view video lessons to learn The Nernst Equation. Or if you need more The Nernst Equation practice, you can also practice The Nernst Equation practice problems.