Question

need help with d.

1. (Step 3: Practice with standard cell potentials) Use the simulation to determine the half-cell potential for the metal "X". a. What is the balanced half-cell reaction corresponding to the reduction of metal X? 2148) 2e- → X Ls) b. What cell potentials did you measure, to help determine the half-cell reduction potential for metal X, and what values did you obtain (list two different cells, and the measured potential)? ZnSO4 i zn V= 1.61 v V = 3.17 Agną i Ag c. What value did you obtain for the half cell reduction potential of metal X?/ Ecent = Ecathode - Eanede 1.61 = -.76 -E anode Eanode 2 -2.374 d. As a check on your answer, use your above value for the half-cell reduction potential of X to calculate the potential of the two cells you measured in part b. Your predicted values should agree with what you measured in part b. Ecel : Z reduction couldalon

use the information above to solve the question for d

Answer 1

1). a). For a small information there is no such metal as X₂ to represent indiviually. In a mixture a metal cation represent as X⁺, X²⁺ like this.

From your question 'a' X_{2 (aq)}+2e^- ---> X _(s)

You can represent itas X²⁺_(aq)+2e^- ---> X _(s)

b). There are such metal cations we have in periodic table like Fe²⁺, Zn^2+,  Cu^2+, Mg^2+...

for your question ZnSO₄ , CuSO₄ .

Zn = -0.76 Cu= 0.34

c). E⁰_cell = E⁰_Zn + E⁰_Cu

_E⁰_cell = 0.34 - 0.76

= -0.42