Additional data needed for this question can be found in Appendix 11 (a) Determine E Zn 2 Zn (at 298 K) for a half cell in which Zn 2 0 25 mol dm 3 (b) Calculate the reduction potential for the half reaction if the ratio of the concentrations of VO 2 V 3 is 1 2 and the pH of the solution is 2 2 Dat...

To solve this question we will use the Nernst equation which relates the reduction potential E of an electrochemical cell at nonstandard conditions to ...

Additional data needed for this question can be found in Appendix 11. (a) Determine E Zn 2+

Question:

Additional data needed for this question can be found in Appendix 11.

(a) Determine E_Zn²⁺/Zn (at 298 K) for a half-cell in which [Zn²⁺] = 0.25 mol dm⁻³.

(b) Calculate the reduction potential for the half reaction:

if the ratio of the concentrations of [VO]²⁺: V³⁺is 1 :2 and the pH of the solution is 2.2.

Data from Appendix 11

The concentration of each aqueous solution is 1 mol dm⁻³ and the pressure of a gaseous component is 1 bar (10⁵ Pa). (Changing the standard pressure to 1 atm (101 300 Pa) makes no difference to the values of E^o at this level of accuracy.) Each half-cell listed contains the specified solution species at a concentration of 1 mol dm⁻³; where the half-cell contains [OH]⁻, the value of E^o refers to [OH⁻] = 1 mol dm⁻³, hence the notation E^o_{[OH⁻] = 1}