Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 3.20 M and [ ] = 0.000100 M Mg(s) + (aq) → (aq) + Fe(s)
E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

Question

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

] = 3.20 M and [ Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 3.20 M and [ ] = 0.000100 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg2+/Mg) = -2.37 V and E°(Fe3+/Fe) = -0.036 V A) -2.24 V B) +2.24 V C) +1.24 V D) -1.24 V E) +2.14 V

] = 0.000100 M Mg(s) + Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 3.20 M and [ ] = 0.000100 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg2+/Mg) = -2.37 V and E°(Fe3+/Fe) = -0.036 V A) -2.24 V B) +2.24 V C) +1.24 V D) -1.24 V E) +2.14 V

(aq) →

(aq) + Fe(s)
E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

Quizplus · Accepted Answer

The Answer of Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 3.20 M and [ ] = 0.000100 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

Calculate the Cell Potential for the Following Unbalanced Reaction That