Final answer:
To calculate the potential of the galvanic cell using the Nernst equation, the specifics of the half-reactions and the number of electrons transferred are needed, which are not provided in the question.
Step-by-step explanation:
To calculate the potential of a galvanic cell with the given reaction at 25°C, we'll use the Nernst equation, which allows us to determine the cell's potential under non-standard conditions. Our reaction is H₂(g) + 2OH⁻(aq) + Sn²⁺(aq) → Sn(s) + 2H₂O(l), and we are given that [OH⁻] = 0.010 M, [Sn²⁺] = 0.020 M, and PH₂ = 1.0 atm. The standard cell potential (E°) is given as 0.97 V. First, write down the standard electrode potentials for the half-reactions and then apply the Nernst equation:
E = E° - (0.05916/n) × log(Q)
Where E is the cell potential, E° is the standard cell potential, n is the number of electrons transferred, and Q is the reaction quotient. However, since the reaction provided does not represent a standard redox reaction in which electrons transfer directly occurs between the reactants and products, direct application of the formula and finding n may not be straightforward.
Here, the question would ideally require the electrode potentials for the specific half reactions involving H₂ and OH⁻ (which would be a reduction), and Sn²⁺ going to Sn(s) (which would be an oxidation). Then, you would combine these two to give the standard cell potential (which is provided), and since we are also given standard conditions for H₂ (PH₂ = 1 atm), we would just need to correct for the non-standard concentrations of OH⁻ and Sn²⁺.