Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.945 M and [ ] = 1.37 M Zn(s) + (aq) → (aq) + Cr(s)
E°(Zn²⁺/Zn) = -0.76 V and E°(Cr³⁺/Cr) = -0.73 V

Question

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [

] = 0.945 M and [ Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.945 M and [ ] = 1.37 M Zn(s) + (aq) → (aq) + Cr(s) E°(Zn2+/Zn) = -0.76 V and E°(Cr3+/Cr) = -0.73 V A) +0.03 V B) -0.03 V C) -1.18 V D) +1.18 V E) +0.49 V

] = 1.37 M Zn(s) + Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.945 M and [ ] = 1.37 M Zn(s) + (aq) → (aq) + Cr(s) E°(Zn2+/Zn) = -0.76 V and E°(Cr3+/Cr) = -0.73 V A) +0.03 V B) -0.03 V C) -1.18 V D) +1.18 V E) +0.49 V

(aq) →

(aq) + Cr(s)
E°(Zn²⁺/Zn) = -0.76 V and E°(Cr³⁺/Cr) = -0.73 V

Quizplus · Accepted Answer

1. Write the half-reactions:
Zn(s) → Zn2+(aq) + 2e-
Cr3+(aq) + 3e- → Cr(s)

2. Determine the standard cell potential, E°cell:
E°cell = E°(Cr3+(aq)/Cr(s)) - E°(Zn2+(aq)/Zn(s))
E°cell = (-0.73 V) - (-0.76 V)
E°cell = 0.03 V

3. Use the Nernst equation to calculate the cell potential, Ecell:
Ecell = E°cell - (0.0592 V/n) x log(Q)
where Q = [Cr3+]/[Zn2+]
Ecell = 0.03 V - (0.0592 V/3) x log(1.37/0.945)
Ecell = +0.03 V

Therefore, the answer is A) +0.03 V. The cell potential is slightly positive, indicating that the reaction can proceed spontaneously in the forward direction.

Calculate the Cell Potential for the Following Unbalanced Reaction That