You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __.

Slides:

Advertisements

Similar presentations

Chpater 4 Oxidation-Reduction

Advertisements

Electrochemical Cells

Unit 11- Redox and Electrochemistry

Unit 7: Redox & Electrochemistry.

Discovering Electrochemical Cells PGCC CHM 102 Sinex.

Voltaic Cells Harnessing the power of Redox Redox Basics Redox Reactions happen when –one substance loses electrons (oxidized) and –one gains electrons.

Electrolytic Cell and Electroplating Chapter 19 Page Chem 12.

A) 80 b) 53 c) 13 d) x 2 = : 10 = 3, x 3 = 309.

Slide 1 of 54  CRS Questions Follow:. Slide 2 of 54 Given the two electrochemical cells to the right, a cell constructed according to the following shorthand.

Lecture 253/27/06 Bottle and Can drive today 11-3 Hagan Info Booth Seminar today at 4 pm.

Lecture 223/19/07. Displacement reactions Some metals react with acids to produce salts and H 2 gas Balance the following displacement reaction: Zn (s)

ELECTROCHEMISTRY. What is Electrochemistry  The branch of chemistry that deals with the use of spontaneous chemical reaction to produce electricity and.

Chapter 13, Preparation to work with cells reaction prediction is a necessary skill 1 st step: Make a list Guidelines: most ionics get listed as (aq) ions.

Electrochemistry Ch. 17. Electrochemistry Generate current from a reaction –Spontaneous reaction –Battery Use current to induce reaction –Nonspontaneous.

Electrochemical cells: utilize relationship between chemical potential energy & electrical energy.

Topic: Electrolytic Cell Do now: p.19 in packet, cross out # 19 and do # 20 and #21. must label anode/cathode.

1 Lec. 2 Faraday’s Laws Lec. 2 Faraday’s Laws Industrial Electrolytic Processes “Electrolysis”

GHS Honors Chem Electro- Chemistry. GHS Honors Chem Electrochemistry Electrochemistry is the study of the relationships between electrical energy and.

Electrochemistry Lesson 8 Electrochemical Cells. Electrochemical cells are Batteries.

Notes on Electrolytic Cells An electrolytic cell is a system of two inert (nonreactive) electrodes (C or Pt) and an electrolyte connected to a power supply.

An Introduction to Electroanalytical Chemistry Electrochemistry: The study of the interchange of chemical and electrical energy Oxidation is the loss of.

Oxidation-Reduction I The Basics A. Definitions 1. Oxidation Loss of electrons Electrons are products (right side) Oxidation number increases ex. Na 0.

Electrochemistry: Oxidation-Reduction Reactions Zn(s) + Cu +2 (aq)  Zn 2+ (aq) + Cu(s) loss of 2e - gaining to 2e - Zinc is oxidized - it goes up in.

Electrolytic Cells Lesson 9 Electrolytic Cells. Notes on Electrolytic Cells An electrolytic cell is a system of two inert (nonreactive) electrodes (C.

Precipitation Titrations Dr. Riham Ali Hazzaa Analytical chemistry Petrochemical Engineering.

Zn │ Zn 2+ ││Cu 2+ │ Cu Std Electromotive Force = Std EMF = Std Cell potential = E° = 1.10 V 2H + + 2e - → H 2 (at 1 atm, 1 M, 25°) Standard EMF = 0 (E°

1. Metals in group 1 have (+1) ox #, group 2 metals (+2) 2. Any single “Pure” element = 0 3. Hydrogen is always (+1) except in metal hydride (-1) LiH.

Hour Exam II Wednesday, March 15 7:00 – 9:00 pm 103 Mumford HallAQG, AQI AllenAQJ BlairAQF 150 Animal Science FisherAQB, AQC KoysAGD PearsonAQA conflict.

Discovering Electrochemical Cells PGCC CHM 102 Sinex.

1http:\\aliasadipour.kmu.ac.ir Electrochemistry

Unit 2: Electrochemistry Electrolysis

Electrolytic Cells. Endothermic.Use electricity to force a nonspontaneous reaction to occur. Endothermic. Electrolytic cells can be identified by the.

14.3 Electrolytic Cells  Electrolysis is the process of converting electrical energy into chemical energy.  Voltaic cells produce electrical energy and.

e- Transfer Theory  Electrons move from the anode to the cathode (from the SRA to the SOA)

Utilizes relationship between chemical potential energy & electrical energy.

Electrochemical cells: utilize relationship between chemical potential energy & electrical energy.

Unit: Chemical Reactions Balancing chemical equations.

U4 S2 L3 Electrolytic cells Textbook Readings MHR page 776: Electrolytic Cells pages : Electrolysis of Molten Salts pages : Electrolysis.

QUESTION For cathodic protection used to prevent corrosion of iron to be effective which of the following must be true? A.The anode used must be a better.

Corrosion of Iron Since E  red (Fe 2+ ) < E  red (O 2 ) iron can be oxidized by oxygen. Cathode: O 2 (g) + 4H + (aq) + 4e -  2H 2 O(l). Anode: Fe(s)

Zumdahl Ch. 17 AP Chemistry

1 UNIT 7 Reduction / Oxidation Reactions “Redox” and Electrochemistry.

CE Chemistry Module 8. A. Involves electron changes (can tell by change in charge) Cl NaBr 2NaCl + Br 2 B. Oxidation 1. First used.

THE ELECTROLYSIS OF AQUEOUS SOLUTION

Redox 21-3 Electrochemistry. 1.) Electrochemical Cells A.) Also called Galvanic Cells B.) Conservation of mass, charge and energy C.) Changes Chemical.

Assigning Oxidation Numbers RULESExamples 2Na + Cl 2  2NaCl Na = 0 or written Na 0 Cl 2 = 0 or written Cl 2 0 RULESExamples 1. Each Uncombined Element.

Nernst Equation  G = -nF  cell  G o = -nF  o cell  G =  cell =  o cell - RT nF ln Q standard non-standard GoGo + RT ln Q.

Redox comes from the two words oxidation and reduction. Oxidation: Loss of electrons. When things lose electrons, they become positive. We learned that.

The Electrolytic Cell. In the electrolytic cell, a nonspontaneous redox reaction is forced to occur by the use of a source of electricity. In the electrolytic.

CHAPTER SIX(19) Electrochemistry. Chapter 6 / Electrochemistry Chapter Six Contains: 6.1 Redox Reactions 6.2 Galvanic Cells 6.3 Standard Reduction Potentials.

General Chemistry Unit 14. A. Involves electron changes (can tell by change in charge) Cl NaBr 2NaCl + Br 2 B. Oxidation 1. First.

To be viewed with PowerPoint. Animation doesn’t work otherwise.

Principles & Modern Applications

14.6 Electrochemistry Unit Review

Reactions of Metals.

Voltaic Cells Aim: To identify the components and explain the functions of an electrochemical (voltaic) cell.

Unit 12 Acids & Bases

Chapter 10 Electrolytic Cells 10.7.

Redox #’s 1-5 #1) The reaction absorbs energy, therefore it is electrolytic (A). #3) Electrolysis requires an external power source (A). #4) Reduction.

utilizes electrical energy to create chemical energy

Redox Reactions battery to start car prevent corrosion

Electrolytic Cells.

Chapter 10 ELECTROLYTIC CELLS 10.7.

!'!!. = pt >pt > \ ___,..___,..

utilizes electrical energy to create chemical energy

Unit 13: Electrochemistry

from a battery or other external energy source

What is a redox reaction?

Presentation transcript:

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __

V __ O 2 bubbled in O 2 ½ cell

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Na +,Cl -

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s)

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr ½ cell

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr ½ cell Cr (s)

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 -

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ OA OA RA --- OA RA OA

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e-

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e- NO 3 - K+K+

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e- NO 3 - K+K+ 1/2O 2(g) +2H + (10 -7 M) + 2e -  H 2 OCr (s)  Cr e -

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e- NO 3 - K+K+ 1/2O 2(g) +2H + (10 -7 M) + 2e -  H 2 OCr (s)  Cr e - + -

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e- NO 3 - K+K+ 1/2O 2(g) +2H + (10 -7 M) + 2e -  H 2 OCr (s)  Cr e /2O 2(g) +2H + (10 -7 M) + 2e -  H 2 OE o red =+0.82V Cr (s)  Cr e - E o ox =+0.74V

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e- NO 3 - K+K+ 1/2O 2(g) +2H + (10 -7 M) + 2e -  H 2 OCr (s)  Cr e (1/2O 2(g) +2H + (10 -7 M) + 2e -  H 2 O)x3E o red =+0.82V (Cr (s)  Cr e - )x2 E o ox =+0.74V

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e- NO 3 - K+K+ 1/2O 2(g) +2H + (10 -7 M) + 2e -  H 2 OCr (s)  Cr e /2O 2(g) +6H + (10 -7 M) +6e -  3H 2 OE o red =+0.82V 2Cr (s)  2Cr e - E o ox =+0.74V

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e- NO 3 - K+K+ 1/2O 2(g) +2H + (10 -7 M) + 2e -  H 2 OCr (s)  Cr e /2O 2(g) +6H + (10 -7 M) +6e -  3H 2 OE o red =+0.82V 2Cr (s)  2Cr e - E o ox =+0.74V + 3/2O 2(g) +6H + (10 -7 M) +2Cr (s)  3H 2 O+2Cr 3+ E o =+1.56V

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e- NO 3 - K+K+ 1/2O 2(g) +2H + (10 -7 M) + 2e -  H 2 OCr (s)  Cr e /2O 2(g) +6H + (10 -7 M) +6e -  3H 2 OE o red =+0.82V 2Cr (s)  2Cr e - E o ox =+0.74V + (3/2O 2(g) +6H + (10 -7 M) +2Cr (s)  3H 2 O+2Cr 3+ )x2 E o =+1.56V 3O 2(g) +12H + (10 -7 M) +4Cr (s)  6H 2 O+4Cr 3+

You try this! Create and label: O 2 ½ cell and Cr (s) ½ cell (neutral conditions) V __ O 2 bubbled in O 2 ½ cell NaCl Pt (s) Cr (s) Cr ½ cell Cr(NO 3 ) 3 Cr 3+, NO 3 - KNO 3 O 2, Na +, Cl -, Pt, K +, NO 3 -, Cr (s), Cr 3+ SOA OA RA --- OA SRA OA Anode Cathode e-e- NO 3 - K+K+ 1/2O 2(g) +2H + (10 -7 M) + 2e -  H 2 OCr (s)  Cr e /2O 2(g) +6H + (10 -7 M) +6e -  3H 2 OE o red =+0.82V 2Cr (s)  2Cr e - E o ox =+0.74V + 3/2O 2(g) +6H + (10 -7 M) +2Cr (s)  3H 2 O+2Cr 3+ E o =+1.56V pH increases Mass decreases corrosion 3O 2(g) +12H + (10 -7 M) +4Cr (s)  6H 2 O+4Cr 3+

And Now, your homework!!!!!