Solution Found!
Consider the following cell diagram:Mg(s)
Chapter 18, Problem 3RC(choose chapter or problem)
Consider the following cell diagram:
\(\mathrm{Mg}(s)\left|\mathrm{MgSO}_{4}(0.40 M) \| \operatorname{NiSO}_{4}(0.60 M)\right| \mathrm{Ni}(s)\)
Calculate the cell voltage at \(25^{\circ} \mathrm{C}\). How does the cell voltage change when (a) \(\left[\mathrm{Mg}^{2+}\right]\) is decreased by a factor of 4 and (b) \(\left[\mathrm{Ni}^{2+}\right]\) is decreased by a factor of 3?
Questions & Answers
QUESTION:
Consider the following cell diagram:
\(\mathrm{Mg}(s)\left|\mathrm{MgSO}_{4}(0.40 M) \| \operatorname{NiSO}_{4}(0.60 M)\right| \mathrm{Ni}(s)\)
Calculate the cell voltage at \(25^{\circ} \mathrm{C}\). How does the cell voltage change when (a) \(\left[\mathrm{Mg}^{2+}\right]\) is decreased by a factor of 4 and (b) \(\left[\mathrm{Ni}^{2+}\right]\) is decreased by a factor of 3?
ANSWER:Step 1 of 3
(a)
The given cell is as follows;
-The anode
- The cathode.