Using Cell Notation and in not more than 2 lines, describe how to make a battery at home from plant source. My Electrolyte = _lemon juice_________________ 1b. Write balanced half-cell and overall equations for the reaction taking place in the described battery in 1. answer= Cu^2+(aq) +2e^- =Cu(s)......(1), E^o=0.34v Zn(s)=Zn^2+(aq) + 2e^-.......(2), E^o=-0.76v 1c. For the cell above, Calculate the standard electrode potential, Eo, for the balanced redox equation. answer for 1c= Ecell=Ecathode - Eanode=0.34-(-)0.76v=1.10v. (i) Compare the calculated Eo to that of the actual [measured] lemon battery above, what is the % difference? (ii) why are they different? (c) calculate the Gibbs Free Enegy, DGo,of actual the lemon cell above (d) Is the cell reaction spontaneous? (d) Why? (e) Calculate the Keq for the cell (f) What is the ratio of the concentration of the [oxidized ion] to that of the [reduced ion] at equilibrium
Can you please solve the d's, e and f? Thanks. I included the answers for the cathode, anode, and Ecell. You can use that to solve the rest of the questions thanks. and also the Eo of actual lemon battery used is 0.906volts
Nernst Equation: E = E° – (RT/nF) ln Q
DGo = -nFEo = -RTlnK
- Using Cell Notation and in not more than 2 lines, describe how to make a battery at home from plant source.
My Electrolyte = _lemon juice_________________
1b. Write balanced half-cell and overall equations for the reaction taking place in the described battery in 1.
answer= Cu^2+(aq) +2e^- =Cu(s)......(1), E^o=0.34v
Zn(s)=Zn^2+(aq) + 2e^-.......(2), E^o=-0.76v
1c. For the cell above,
- Calculate the standard electrode potential, Eo, for the balanced redox equation.
answer for 1c= Ecell=Ecathode - Eanode=0.34-(-)0.76v=1.10v.
(i) Compare the calculated Eo to that of the actual [measured] lemon battery above, what is the % difference?
(ii) why are they different?
(c) calculate the Gibbs Free Enegy, DGo,of actual the lemon cell above
(d) Is the cell reaction spontaneous?
(d) Why?
(e) Calculate the Keq for the cell
(f) What is the ratio of the concentration of the [oxidized ion] to that of the [reduced ion] at equilibrium
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