Calculate the value of E_cell for a zinc-platinum electrochemical cell when the concentration of Pt²⁺(aq) is 0.050 M and the concentration of Zn²⁺(aq) is 1.1 M. E^$\circ$_cell = 1.96 V under standard conditions. Pt is the less active metal.

Question

Quizplus · Accepted Answer

The Nernst equation can be used to calculate the cell potential under non-standard conditions: EF1F1F1S1F1F1F10_cell = EF1F1F1S1F1F1F10_cell + (0.0592 V/pH) log(Q), where Q is the reaction quotient. For this cell, the balanced equation is: Zn (s) + Pt2+ (aq) → Zn2+ (aq) + Pt (s) So Q = [Zn2+]/[Pt2+]. Plugging in the given concentrations and the standard potential, we get: EF1F1F1S1F1F1F10_cell = 1.96 V Q = [Zn2+]/[Pt2+] = (1.1 M)/(0.050 M) = 22 EF1F1F1S1F1F1F10_cell = 1.96 V EF1F1F1S1F1F1F10_cell = 1.96 V + (0.0592 V/pH) log(22) = 1.92 V Therefore, the answer is D, 1.92 V.

Calculate the Value of Ecell for a Zinc-Platinum Electrochemical Cell ∘\circ∘

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