CuS+HNO 3 →Cu(NO 3 ) 2 + S + NO+H 2 O. CuS -2 +HN +5 O 3 →Cu(NO 3 ) 2 + S 0 + N +2 O+H 2 O.

Slides:

Advertisements

Similar presentations

Chemical Reaction parts are mixed together to make something new.

Advertisements

KJ + Cu(NO 3 ) 2 → CuJ + J 2 + KNO 3 KJ + Cu(NO 3 ) 2 → CuJ + J 2 + KNO 3.

Ag + H 2 S  Ag 2 S + H 2 Ag-Ag- H-H- S-S-. 2Ag + H 2 S  Ag 2 S + H 2.

H 2 S(g) + 2 O 2 (g)  SO 3 (g) + H 2 O(l) H 2 S(g) + 2 O 2 (g)  H 2 SO 4 (l) ΔH = kJ H 2 SO 4 (l)  SO 3 (g) + H 2 O(g) ΔH = kJ H 2 O(g)

Drill – 2/28/11 Sodium chloride decomposes into sodium and chlorine. How much (in grams) sodium chloride is required to produce 50.0g of chlorine gas?

1. Write a sentence that describes

This work is licensed under a Creative Commons Attribution-Noncommercial-Share Alike 2.0 UK: England & Wales License REDOX reactions.

Electron-Transfer Reactions Cu 2+ (aq) + Zn(s)  Cu(s) + Zn 2+ (aq)

Electron-Transfer Reactions Cu 2+ (aq) + Zn(s)  Cu(s) + Zn 2+ (aq)

Balancing Chemical Equations. CA Standards Students know how to describe chemical reactions by writing balanced equations.

Balancing Chemical Equations

Chemical Equations. A Chemical Reaction Reactants Products Yields (produces)

Balancing redox reactions

Free Energy and Cell Potential.  G o = - nF  o Faraday (F) = the charge of 1 mole of electrons q = nFw = -q  heat work.

WE BE COOKING…. Stoichiometry. Deals with the chemistry of quantifying chemical reactions through the use of:  Balancing equations  Moles (mol)  Molarity.

两会协议执行成果总结回顾 2014 年 2 月. 时间地点协议或共识协议或共识第一次会谈 2008 年 6 月 13 日北京海峡两岸包机会谈纪要海峡两岸关于大陆居民赴台湾旅游协议第二次会谈 2008 年 11 月 4 日台北海峡两岸空运协议海峡两岸海运协议海峡两岸邮政协议.

Balancing Redox Equations

Page 16.  Some Transition Metals can form more than one type of cation. For example, copper can have either a +1 or a +2 charge  Iron can have either.

Note: If the cation has a Roman numeral, you MUST include the correct Roman numeral!

Balancing Redox Reactions. Steps: 1.Assign oxidation numbers 2.Write half reactions 3.Balance electrons to determine coefficients needed.

Ring stand round bottom flask iron ring pre-1982 penny clamp rubber stopper tubing graduated cylinder.

Helpful Definitions Solutions: homogeneous mixture of two or more substances physically mixed together in a uniform way. Solute: substance being dissolved.

Section 4.4 Oxidation Reduction Reactions Redox Reactions Electron-Transfer Reactions.

Oxidation/Reduction Reactions REDOX REACTONS! All chemical reactions fall into two categories those that are redox and those that are not redox! Redox.

Electrochemistry A lemon can power a small light bulb. Where does the energy come from? RedOx reactions move electrons from one element to another.

1 AnodeCathode Basic Concepts of Electrochemical Cells.

Chemical Nomenclature (or how we name compounds!) 1. binary ionic (cation + anion) 2. molecular (covalent) compounds (anion + anion) 3. ternary ionic.

Copper Minerals a % composition exercise. Simple Copper Sulfides Chalcocite: copper (I) sulfide Tenorite: copper (II) sulfide 1. Write the formulas for.

Modern Chemistry Chapter 8 Chemical Equations and Reactions

Electrochemistry Electrolysis.

Chapter 18 Notes1 3. standard reduction potentials by convention, half-reactions are written as reductions; to get the overall reaction, use right electrode.

Nernst Equation Walther Nernst

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.

© 2012 Pearson Education, Inc. Oxidation-Reduction Reactions An oxidation occurs when an atom or ion loses electrons. A reduction occurs when an atom or.

REDOX REACTIONS Oi L Oxidation is L osing electrons (becomes more positive) Ri G Reduction is G aining electrons (becomes less positive) Cu(s) + 2AgNO.

Film Appreciation 124. Uninterrupted sequence of frames.

Bright Yellow Ppt Rusty Red Ppt No Rxn Creamy Ppt Coffee Brown Ppt

Oxidation and Reduction By the end of this lesson, you should be able to: 1.State that a metal element reacting to form a compound is an example of oxidation.

AZOT. Nitrogen was discovered by Daniel Rutherford at 1772 in Scotland. Origin of name: from the Greek words "nitron genes" meaning "nitre" and "forming"

25 December Fraser Sockeye Life Cycle Diagram

Redox Reactions: HALF REACTIONS

BALANCING EQUATIONS WHERE ELEMENTS APPEAR IN MORE THAN ONE PRODUCT SPECIES Example: Copper metal + Nitric Acid → Copper Nitrate + Nitrogen Dioxide + Water.

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 1 Chapter 15 Oxidation- Reduction: Transfer of Electrons 15.1 Oxidation and Reduction Rust forms.

Lab: From Copper to Copper Investigation 4-E p Chemistry, Clancy et al.

Electrochemistry Oxidation-reduction reactions. Review Ionic bonds : give and take of electrons (example NaCl) Ionic bonds : give and take of electrons.

Double Replacement Reactions Section 4.5. Driving Force – Two compounds  There must be a driving force for the reaction to take place, otherwise it will.

Who wants to be a millionaire?. 2 Ag + (aq) + Hg (l) > 2 Ag (s) + Hg 2+ (aq) 1. For the given reaction, What is being oxidized?

Chemical Reactions Unit 7 1. Chemical Equations 2 Combustion Reactions A substance reacts with O 2 (typically with the help of a flame) 2 C 4 H

Electrolysis of Copper Chloride Solution. What is a solution?

3.1.7 Redox. A redox reaction is one in which both reduction and oxidation take place at the same time. The original definition of oxidation was the formation.

Unit 08 Part C Questions Reduction - Oxidation Day 1: Questions # 1-17 Day 2: Questions # Day 2: Questions #

Limiting Reactants Unit 7 1. Limiting Reactants 2.

Types of Chemical Reactions 20 point total Decomposition ABC A + B + C One reactant multiple products.

1 Pb(NO 3 ) 2 (aq) + KI (aq)  PbI 2 (s) + KNO 3 (aq) __ 212 Molarity and Stoichiometry M M V V P P mol M L M = mol L mol = M L What volume of 4.0 M KI.

Describing Chemical Reactions Prentice-Hall Chapter 11.1 Dr. Yager.

Challenge Stoichiometry Lesson 7. A 10.0 g sample of a Cu/Ag alloy reacted with concentrated HNO 3 according to the following equations. A total of

Lab 1 General protein color tests

Balancing Redox Equations

Balancing Redox Equations

Definitions *Amino Acids (a.a):

Hn is the number of moves to solve. n = 1, Hn = 1 n = 2, Hn = 3 n = 3, Hn = 7 Hn = 2Hn

Predicting Redox Reactions 9.3.

Predicting Redox Reactions 9.3.

COUNTING ATOMS Example #1 Example #2 NaOH Na – 1 atom O - 1 atom

Balancing Redox Equations

І. Ұйымдастыру кезеңі Сәлеметсіздерме оқушылар! Сыныпта кезекші кім?

Challenge Stoichiometry

Write the oxidation numbers for each of the following:

Practice How many grams of H2O are produced by completely reacting 24 g of O2? 2 H2 + O2  2 H2O convert to moles  convert to the desired molecule  convert.

Chemical Formulas Quiz- 10/7/15

Presentation transcript:

CuS+HNO 3 →Cu(NO 3 ) 2 + S + NO+H 2 O

CuS -2 +HN +5 O 3 →Cu(NO 3 ) 2 + S 0 + N +2 O+H 2 O

CuS+HNO 3 →Cu(NO 3 ) 2 + S + NO+H 2 O CuS -2 +HN +5 O 3 →Cu(NO 3 ) 2 + S 0 + N +2 O+H 2 O N e → N +2

CuS+HNO 3 →Cu(NO 3 ) 2 + S + NO+H 2 O CuS -2 +HN +5 O 3 →Cu(NO 3 ) 2 + S 0 + N +2 O+H 2 O N e → N +2 S -2 – 2e → S 0

CuS+HNO 3 →Cu(NO 3 ) 2 + S + NO+H 2 O CuS -2 +HN +5 O 3 →Cu(NO 3 ) 2 + S 0 + N +2 O+H 2 O N e → N +2 S -2 – 2e → S

CuS+HNO 3 →Cu(NO 3 ) 2 + S + NO+H 2 O CuS -2 +HN +5 O 3 →Cu(NO 3 ) 2 + S 0 + N +2 O+H 2 O N e → N +2 S -2 – 2e → S

CuS+HNO 3 →Cu(NO 3 ) 2 + S + NO+H 2 O CuS -2 +HN +5 O 3 →Cu(NO 3 ) 2 +3S 0 +2N +2 O+H 2 O N e → N +2 S -2 – 1e → S

CuS + HNO 3 →Cu(NO 3 ) 2 + 3S +2NO + H 2 O 3CuS + HNO 3 → Cu(NO 3 ) 2 + 3S+ NO + H 2 O 3CuS + HNO 3 → 3Cu(NO 3 ) 2 + 3S + 2NO + H 2 O

3CuS +8HNO 3 → 3Cu(NO 3 ) 2 +3S +2N O+H 2 O 3CuS + 8HNO 3 → 3Cu(NO 3 ) 2 + 3S + 2NO + 4H 2 O