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 sub-parts d,e and f? Thanks. The other parts have already been solved please dont solve them!! Solve just the subparts D,E AND F! Thanks...
Eo of lemon juice used=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.
1c. For the cell above,
- Calculate the standard electrode potential, Eo, for the balanced redox equation.
(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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