Write the standard line notation for each cell below.
Mn2+ + 2 e- --> Mn E = -1.18 V
Fe3+ + 3 e- --> Fe E = -0.036 V
These are only half cells.
Mn^2+|Mn
Fe^3+|Fe
To write the standard line notation for these cells, you need to follow the general format:
oxidized species (reducing agent) + n e- --> reduced species (oxidizing agent) E = standard cell potential
Let's write the standard line notation for each cell:
1. For the oxidation half-reaction: Mn2+ --> Mn
For the reduction half-reaction: 2 e- --> 2 e-
Combine the half-reactions: Mn2+ + 2 e- --> Mn
Add the standard cell potential: E = -1.18 V
The standard line notation is: Mn2+ + 2 e- --> Mn E = -1.18 V
2. For the oxidation half-reaction: Fe3+ --> Fe
For the reduction half-reaction: 3 e- --> 3 e-
Combine the half-reactions: Fe3+ + 3 e- --> Fe
Add the standard cell potential: E = -0.036 V
The standard line notation is: Fe3+ + 3 e- --> Fe E = -0.036 V
Remember, in the line notation, the oxidized species (reducing agent) is written on the left side, and the reduced species (oxidizing agent) is written on the right side. The number of electrons involved in each half-reaction is balanced, and the standard cell potential (E) is specified at the end.