Ch13 Fundamentals of Electrochemistry (by Prof. Myeong Hee Moon)

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Ch13 Fundamentals of Electrochemistry (by Prof. Myeong Hee Moon)

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Ch. 13 13 Fundamentals of Electroc Electr ochemis hemis 13-1. Basic Concepts of electrochemistry redox reaction reaction : reactions wi th electron transfer oxidized : los es electrons reduced : gains electrons Fe3+ + V2+



Fe2+ + V

oxidizing agent agent (oxidant) (oxidant) : takes takes electrons electrons from others and reduce reducing agent (reductant) : oxidizes itself

1. Electric charge (q) q : [co ulo mb] or [C] = 1.60 1.602 2 x 10-19 C for a sin gle electro for 1 mole of e

q = n F

13:20

1.602 x 10-19 C x 6.02x1023 /mol 9.649x10 4 C/mol

Faraday constant [F]

Anal. Chem. by Prof. Myeong Hee Moon

133-1. 1. Basic Conce Conc epts of electrochemis electro chemistry try 2+ was Master your with Scribd ex) semester If 5.585 5.585 g o f Fe reduced in th e reaction reaction abov e, how m any Read Free Foron 30this Days Sign up to vote title 2+ coulombs of charge must h ave bee been n transferred transferred from V to Fe3+? & The New York Times  Useful  Not useful

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13-1. Basic Concepts of electrochemistry 2. Electric Current : quantity of charge per second [A] , ampere ex) Suppose that electrons are forc ed int o a platin um wire immersed in a solution cont aining Sn 4+, which is reduced to Sn 2+ at a constant rate of 4.24 mmol/h. How much current flows into the solution ?

0.227 C/s = 0.227A

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13-1. Basic Concepts of electrochemistry 3. volsemester tage, wor k, with free energy Master your Scribd difference in electrical potential (E) between Read Free Foron 30this Days Signtwo up topoints vote title & The New York Times  Useful  Not useful = potential difference Special offer for students: Only $4.99/month.

[V], volts work : energy in joules [J]

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13-1. Basic Concepts of electrochemistry The free energy change : G work done on surrounding : - G G = -E q = - n F E

4) Ohm's law

I 

current, I, flowi ng throug h a circ uit

E

[ ]

R

13:20





13-1. Basic Concepts of electrochemistry

Master your semester with Scribd  Read Free For 30 Days Sign up to vote on this title 5) pow er : p work done per unit time, J/s or watt  & The New York Times  Useful  Not useful Special offer for students: Only $4.99/month.

work Eq

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q

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13-1. Basic Concepts of electrochemistry Type of Electroc hemical cells

Galvanic Cells : A cell generates electr ic energy from where ? chemic al reaction. = spon taneous reactio Electroly tic Cells : requi res an external so urce of E.E. one reagent mus t be oxid ized, the other reduced.

13:20





13-2. A galvanic cell in Acti on

Master your semester with Scribd reduct ion : & The New York Times Special offer for students: Only $4.99/month.

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Read Free For Days Sign up to 2 vote 2AgCl (s) + e-on30this 2title Ag(s) +  2 Cl  Useful  Not useful Cancel anytime. oxi dation : Cd(s) Cd2+ (aq) + 2 e -

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13-2. A galvanic c ell in Actio n KCl cont ained gel agar wit

2. Salt Bridge

cathod e: 2 Ag + (aq) + 2 e2 Ag(s) 2+ anode : Cd (s) Cd (aq) + 2 e net : Cd(s) + 2 Ag +(aq) Cd 2+ + 2 Ag(s) 13:20

3) Line notation | phase boun dary || salt bridge

Cd(s) | Cd(NO3)2 (aq) || AgNO3 (aq) | A Anal. Chem. by Prof. Myeong Hee Moon




13-3. Standard Potentials

Master your semester Scribd measured vol tage with potent ial difference between Ag and Cd  electr Read Free Foron 30this Days Sign up to vote title  & The New York Times Useful Not useful   - Positive voltage when e- flows Special offer for students: Only $4.99/month.

from anode into n eg terminal.

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13-3. Standard Potentials

Standard Reduction Potentials std. Reductio n pot ential = potential di fference between the std potential of th e reduction of int erest and the potential of SHE

positive: electrons move from SHE to Ag + negative: electrons moves reverse direction

13:20





13-4. Nerns t eq : net dri ving for ce 1) Nernst eq. for a half reactio n, Master your semester with Scribd a A + n eb B & The New York Times Special offer for students: Only $4.99/month. RT

E  E0 

b B

A log

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  Cancel anytime. : std .reduction potential R: gas cons tant 8.314 J/mol-K E0

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13-4. Nerns t eq : net dri ving for ce 2) Nerns t equation f or a compl ete reaction vol tage difference (E) for t he two electrod es. E = E+ - EE+ : potential of electrode at positi ve input terminal of potentiometer = Ecathode

Procedure: 1. wri te half reactions w ith S.R.P. 2. wri te Nernst equation fo r half reaction 3. The more pos iti ve E0 reduction predominantly happen 4. calcul ate net cell vol tage E = E+ - E5. write balanced reaction by subtracting the half reaction

13:20





13-4. Nerns t eq : net dri ving for ce

ex) Findsemester the voltage ofwith the cell in Figure 14-5 if the right half cell contains 0.50 Master your Scribd  Read Free For 30 Days Sign up to vote on this title AgNO3 (aq) and the left half cell contains 0.010 M CdCl 2 (aq). Write the  net & The New York useful direction  Useful reaction and Times state whether it is spontaneous in the forwardorNot reverse Special offer for students: Only $4.99/month.

right: 2 Ag + (aq) + 2 e-

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2 Ag (s)

0.799V

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13-4. Nerns t eq : net dri ving for ce * Advice for finding relevant half-cell reactions

Pb(s) | PbF2 (s) | F- (aq) || Cu +2 (aq) | Cu(s) anode oxidation right : left:

Cu2+ + 2 e PbF2 (s) + 2 e

cathode reduction

Cu (s) 2 F- + Pb (s)

in fact, 2 F- + Pb (s)

13:20

PbF2 (s) + 2 e





13-5. E0 and the equilibrium constant E and the equilibrium constant Master your semester with Scribd : galvanic cell produces electric ity & The New York Times 0

At$4.99/month. eq. E=0 Special offer for students: Only

righ t electrode : a A + n e-


until th e cell eq. Usefulreaches  Not useful Cancel anytime. cC

E+0

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13-6. Cells as chemical prob es

Ag + (aq) + Cl -(aq) CH3COO- (aq) + H+(aq)

right half cell : AgCl(s) left half cell : CH3COOH

they come to equilibrium without other half-cell --- c hem ic al r eac ti on 13:20






Master your semester with cell assembled,with Scribd Ag Cl(s ) + e Ag (s) & The New York Times Special offer for students: Only $4.99/month.

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in left : the only element -- hydrogen gas bubbles out

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ex) The cell in the following figure measures the formation constant (Kf ) of Hg(EDTA)2-. The solution in the right hand compartment contains 0.500 mmol o Hg2+ and 2.00 mmol of EDTA in a volume of 0.100 L buffered to pH 6.00. If the voltage is 0.331V, find the value of K f for Hg(EDTA)2-.

13:20





Master your semester with Scribd Selected Problem No. & The New York 14-4, -5, Times -10, -17, -35, -38, Special offer for students: Only $4.99/month.


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Ch13 Fundamentals of Electrochemistry (by Prof. Myeong Hee Moon)

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