MasteringChemistry: Assignment 6 Electrochemistry-Part 1 Google Chrome D session

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MasteringChemistry: Assignment 6 Electrochemistry-Part 1 Google Chrome D session.masteringchemistry.com 38170463 Signed in as Craig Hogard Help I Close CHEM 1121 FALL 2014. Assignment 6 Part The Nernst Equation Resources previous l 10 of 15 l next The Nernst Equation Part A The Nernst equation is the one of the most important Using the reaction and the E given below equations in electrochemistry. At standard temperature, 25 C or 298 K, the equation has the form 2Co (aq) +2C aq)-- 2Co (aq) Cl2(g) EP 0.46 V 0.0591 E-E logQ what is the cell potential at 25 C if the concentrations are Co3+ o.158M. [Co2+ 4.00x10-3M. and Cl 0.510 Mand the pressure of where E is the standard reduction potential for the reaction in volts and C is reaction quotient. reaction Cla is P 3.30atm Express your answer numerically in volts. has the usual form reactants A table of standard reduction potentials gives the voltage at standard conditions 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Submit Hints My Answers Give Up Review Part Provide Feedback Continue 12:13 PM 10/27/2014

Explanation / Answer

I answered a similar question earlier today, but with different values than you have given.
I looked up the following standard reduction potentials, E^o, on the web:

A) Co+3 + e- ==? Co+2 +1.82
B) 2e + Cl2 ==? 2Cl- +1.36
Reverse B: 2Co+3 + 2Cl- =? 2Co+2 + Cl2 E^o = 0.46
I do not see how the value of 0.71 V was obtained.

E = E^o - 0.0592/n log Q ; n =2 since it is two electron change Q = [CO+2]^2PCL2 / [CO+3]^2 [ CL-2]^2
E= +0.46 - 0.059/ 2 * log (3.30)(4 X 10-3)^2 / (0.510)^2(0.158)^2

E= 0.521

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