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. II and III
c. II only
d. III only
e. I only
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