Consider a hydrogen reduction electrode represented as H ⁺ (aq) | H ₂ (g) | Pt . Read the following four statements regarding its reduction potential at 298 K: I. The reduction potential increases (becomes less negative) as the pH of the solution decreases at constant pressure. II. The reduction potential becomes more negative if the pressure of H ₂ gas is increased at constant pH. III. At pH = 10 and P_ H ₂ = 1 atm,

Step-by-step solution

The reduction half-reaction is: 2 H ⁺ (aq) + 2 e ⁻ H ₂ (g) Using the Nernst equation for reduction potential: E_ red = E^ - 0.059 2 P_ H ₂ [ H ⁺]^2 E_ red = -0.059 pH - 0.059 2 P_ H ₂ Statement I: As pH decreases, the term -0.059 pH becomes less negative, so the reduction potential increases. (Correct) Statement II: As P_ H ₂ increases, the term - 0.059 2 P_ H ₂ becomes more negative, decreasing the reduction potential. (Correct) Statement III: At pH = 10 and P_ H ₂ = 1 atm: E_ red = -0.059 10 - 0 = -0.59 V. (Corre