1. …at the Sn electrode as tin atoms turn into tin ions the mass of the electrode decreases
and the tin ions go into the solution!

2. ◄K+
NO3- ◄

3. The cell potential will remain the same as the reaction quotient, Q, in the Nernst Equation will have the value of 1.
It will last less time as equilibrium will be established sooner. You could also say that the copper (II) ions will be exhausted in less time as there are less of them.

4. Write the line notation describing this cell.
(e) Calculate the standard cell potential for the reaction.
Cu e-  Cu E° = 0.34 V
Sn°  Sn e E° = 0.14 V
E°overall = 0.48 V
Write the overall reaction equation for which this is the standard cell potential.
Cu2+ + Sn  Cu + Sn2+
Write the line notation describing this cell.
Sn│Sn2+ ǁ Cu2+│Cu

5. You can’t tell unless the actual current is given.
(f.) If an electric current was forced through the cell opposite of the spontaneous process, which metal would plate out on the cathode? If the current ran for 5.0 minutes, how much of that metal would have been added to the cathode?
The tin would plate out.
You can’t tell unless the actual current is given.
If the current was 2.5 A, how much of the metal would have plated out?
( s)(2.5 A)(1 mol e-/96500 A s)(1 mol Sn/2 mol e-)
(118.7 g/mol Sn)
= 0.46 g Sn