Download presentation

Presentation is loading. Please wait.

Published byGillian Chapp Modified over 2 years ago

1
CHAPTER 16 (pages 776-792) 1.Oxidation and Reduction 2.Galvanic Cells, Half Reactions (E° anode & E° cathode ) 3.Standard Reduction Potential (E°) 4.Nernst Equation, and the dependence of Potential on Concentration 5.Relationship between Equilibrium Constant and Standard Potential 6.Driving Force, ΔG and ε 1

2
REDOX REACTIONS MnO 2 + 4 HBr MnBr 2 + Br 2 + 2 H 2 O 3 H 2 S + 2 NO 3 – + 2 H + S + 2 NO + 4 H 2 O 2

3
OBSERVED REDOX PROCESSES 3

4
GALVANIC CELLS 4

6
INERT ELECTRODES 6

7
STANDARD REDUCTION POTENTIALS 7

8
8

9
MEASURING STANDARD POTENTIALS 9

10
CALCULATING STANDARD CELL POTENTIAL Al (s) + NO 3 − (aq) + 4 H + (aq) Al 3+ (aq) + NO (g) + 2 H 2 O (l) 10

11
ADDITIONAL EXAMPLE Fe (s) + Mg 2+ (aq) Fe 2+ (aq) + Mg (s) 11

12
ox: Fe( s ) Fe 2+ ( aq ) + 2 e − E = +0.45 V red: Pb 2+ ( aq ) + 2 e − Pb( s ) E = −0.13 V tot: Pb 2+ ( aq ) + Fe( s ) Fe 2+ ( aq ) + Pb( s ) E = +0.32 V

13
ELECTROMOTIVE POTENTIAL 13

15
E° CELL, Δ G° AND K Under standard state conditions, a reaction will spontaneously proceeds in the forward direction if: –Δ G° < 1 (negative) – E° > 1 (positive) – K > 1

16
Design a voltaic cell with the following half cells and complete the calculations: Ag + (aq) + 1e - Ag (s) E o = 0.80 V Pb 2+ (aq) + 2e - Pb (s) E o = -0.13 V a.Calculate the E o cell (potential at standard conditions) b.Calculate G o. c.Calculate d.Calculate the E cell if [Ag + ] = 2.0 M and [Pb 2+ ] = 1.0 x 10 -4 M.

17
Williams, spring 2009 stop here

18
Design a voltaic cell with the following half cells and complete the calculations: Ag + (aq) + 1e - Ag (s) E o = 0.80 V Pb 2+ (aq) + 2e - Pb (s) E o = -0.13 V Calculate the E o cell (potential at standard conditions)

19
Design a voltaic cell with the following half cells and complete the calculations: Ag + (aq) + 1e - Ag (s) E o = 0.80 V Pb 2+ (aq) + 2e - Pb (s) E o = -0.13 V Calculate G o.

20
Design a voltaic cell with the following half cells and complete the calculations: Ag + (aq) + 1e - Ag (s) E o = 0.80 V Pb 2+ (aq) + 2e - Pb (s) E o = -0.13 V Calculate

21
Design a voltaic cell with the following half cells and complete the calculations: Ag + (aq) + 1e - Ag (s) E o = 0.80 V Pb 2+ (aq) + 2e - Pb (s) E o = -0.13 V Calculate the E cell if [Ag + ] = 2.0 M and Pb 2+ ] = 1.0 x 10 -4 M.

23
OBJECTIVE 11.4: PROVIDE A THOROUGH OVERVIEW OF APPLICATIONS OF ELECTROCHEMICAL CELLS INCLUDING FUEL CELLS, CORROSION, AND OTHER TOPICS AS TIME PERMITS. 23

24
CORROSION corrosion is the spontaneous oxidation of a metal by chemicals in the environment since many materials we use are active metals, corrosion can be a very big problem

25
RUSTING rust is hydrated iron(III) oxide moisture must be present electrolytes promote rusting acids promote rusting – lower pH = lower E° red

26
Dry Cell Batteries

27
Lead – Acid Storage Battery

28
Biological Electrochemistry

29
Lithium Ion Battery

Similar presentations

OK

Created by C. Ippolito March 2007 Updated March 2007 Chapter 22 Electrochemistry Objectives: 1.describe how an electrolytic cell works 2.describe how galvanic.

Created by C. Ippolito March 2007 Updated March 2007 Chapter 22 Electrochemistry Objectives: 1.describe how an electrolytic cell works 2.describe how galvanic.

© 2017 SlidePlayer.com Inc.

All rights reserved.

Ads by Google

Ppt on first conditional exercises Ppt on revolt of 1857 images Ppt on power factor meter Ppt on statistics in maths the ratio Ppt on team building activities Ppt on australian continental divide Ppt on programmable logic array examples Ppt on save heritage of india Download ppt on mind controlled robotic arms for sale Ppt on summary writing skills