Question

Consider the following unbalanced equation. H1+(aq) + Fe(s) → H2(g) + Fe2+ (aq) (a) What are the following standard voltages? Includeţthe sign. Change the sign as allowed by the data in the table. standard oxidation potential for the oxidation half-cell .00 X V reduction potential for the reduction half-cell .44 X V potential for the entire cell (b) Select all that apply for the reaction under standard conditions. Hl+ is the substance being oxidized. Fe is the substance being oxidized. Hl+ is the substance being reduced. Fe is the substance being reduced. The forward reaction is spontaneous. The reverse reaction is spontaneous. Electrons will flow from the H half-cell to the Fe half-cell. Electrons will flow from the Fe half-cell to the H half-cell. [H1+] increases as the cell operates. [H1+] decreases as the cell operates. [Fe2+ ] increases as the cell operates. [Fe2+] decreases as the cell operates. [H1+] and [Fe2+] remain constant.

Answer 1

The standard reduction potential of Fe²⁺ is -0.44 so oxidation potential is 0.44.

The standard reduction potential of H⁺ is 0.0

E_{cell(standard)} = E_{cell(standard) ox. Fe} + E_{cell(standard) red. H}

0.44+0 = 0.44

ΔG° is negative = spontaneous reaction

ΔG° = -nFE°

E° = positive

ΔG° = negative

Reaction spontaneous

Fe oxidised

H⁺ reduced, decreased

Fe²⁺ increased

Electron flow from Fe half cell to H⁺ half cell.