Question

The following galvanic cell at standard conditions has a potential of 0.03 V:
Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s).
What would be the effect of increasing the concentration of Ag+?

A. The cell potential will be 0 V.
B. The cell potential will decrease.
C. The cell potential will not change.
D. The cell potential will increase.

Answer 1

@nechirwan Help!

Answer 2

Use the Nernst equation: \(\xi=\xi^o+\dfrac{RT}{nF}ln(\dfrac{[Fe^{2+}]}{[Ag^+]}{}) \)

At 25 celsius: \(\xi=\xi^o+\dfrac{0.0592}{n}log(\dfrac{[Fe^{2+}]}{[Ag^+]}{}) \)


you basically wanna compare the values you get by changing the concentration, so

At std cond, \([Fe^{2+}]=[Ag^+]=1\), therefore \(log\dfrac{1}{1}=0\)

the cell potential is 0.03V

When \([Ag^+]\) is increased, \(log\dfrac{1}{2}=-0.3010\)

if you work it into the equation you'll notice the voltage increased.

Answer 3

by the way i messed up the second equation, it should be:

\(\xi =\xi^o-\dfrac{0.0592}{n}log\dfrac{[Fe^{2+}]}{[Ag^+]}\)