Question

Calculate the standard cell potential, ∘cell, for the equation Sn(s)+F2(g)⟶Sn2+(aq)+2F−(aq) Use the table of standard reduction potentials.

Answer 1

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.

Answer 2

The standard cell potential for the given equation is +2.73 V.

Step-by-step explanation:

The standard cell potential, symbolized as E°cell, can be calculated using the standard reduction potentials provided in the table. In the given equation, Sn(s) + F2(g) ⟶ Sn2+(aq) + 2F-(aq), we need to find the reduction potentials for each half-cell. The reduction potential for Sn2+ is given as +0.14 V, and the reduction potential for F- is given as +2.87 V. To calculate the standard cell potential, we subtract the reduction potential of the anode (Sn2+) from the reduction potential of the cathode (F-) to obtain the overall cell potential. Therefore, the standard cell potential for this equation is +2.87 V - (+0.14 V) = +2.73 V.