Final answer:
The standard cell potential, ∘cell, for the equation Sn(s)+F2(g)⟶Sn2+(aq)+2F−(aq), is +3.01 V.
Step-by-step explanation:
To calculate the standard cell potential, ∘cell, for the given equation Sn(s)+F2(g)⟶Sn2+(aq)+2F−(aq), we need to use the table of standard reduction potentials. According to the table, the reduction potential for Sn2+(aq) is -0.14 V and the reduction potential for F−(aq) is +2.87 V.
Since F−(aq) has a higher reduction potential than Sn2+(aq), it will undergo reduction within the cell. Therefore, the oxidation half-cell will consist of Sn(s) and the reduction half-cell will consist of F2(g).
The standard cell potential is the difference between the potentials of the reduction and oxidation half-cells. In this case, it is (+2.87 V) - (-0.14 V) = +3.01 V.