electrochemistry HW help?

Question

Answer any of them if you can please

n = 9 and E° = 0.522v for a redox reaction with E = 0.596v. Calculate pQ. Assume T = 298.15K. Answer tolerance: ±0.01

A metal undergoes electrolytic reduction according to ne- + Mn+ ===> M. What current (in Ampères) must be provided to deposit the metal at a rate of 0.114 mol/hr if n = 1?

What is pK for a REDOX reaction under standard conditions if n = 5 and E° = -0.435v? Error tolerance: ±0.01

Answer 1

Lancenigo di Villorba (TV), Italy

QUESTION 1)
The Nernst-Standard Potential formula

E = E° + (R * T / (n * F)) * LN(Q)

leads to

Q = EXP((E - E°) * n * F / (R * T)) =
= EXP((0.596 - 0.522) * 9 * 96,500 / (8.3 * 298.16)) =
= 1.9E+11

QUESTION 2)
During an electroplating experiment

Mn+(aq) + ne ---> M(s)

a metallic coating was layed.
Referred to Mono-valent Metallic Salts, the Molar Rate have to be 0.114 mol/hour. I will apply the Faraday's Laws of Coulometry

0.114 * n * F = 0.114 * 1 * 96,500 = 11,001 C/hour = 3 A

since "1 A" or 1 Ampére is the electrical current able to carry out 1 C during 1 s.

QUESTION 3)
A Redox Reaction interests this latter trouble.
Since the question refer to Equilibrium's Constant, it refer also to Equilibrium's Conditions.
Since I assume to avoid any dissipative phenomena, at these conditions

E = 0 V

which it turns in the Nernst' Equation

0 = E = E° + (R * T / (n * F)) * LN(K)

K = EXP(0 - E° * n * F / (R * T)) =
= EXP(0 - (-0.435) * 5 * 96,500 / (8.3 * 298.16)) = 6.1E+36

I hope this helps you.

Answer 2

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Answer 3

For the third one, DGo (standard delta G) is related to both E and K. So from those two relationships, RTlnK=-nFE

You can solve for K and then find pK.

Sorry I can't hope you with the others...it's been too long.