Steps for balancing a chemical equation

Size: px
Start display at page:

Download "Steps for balancing a chemical equation"

Transcription

1 The Chemical Equation: A Chemical Recipe Dr. Gergens - SD Mesa College A. Learn the meaning of these arrows. B. The chemical equation is the shorthand notation for a chemical reaction. A chemical equation shows the molar quantities of reactants and products in a reaction. react to produce 1Reactants 1Products the number out in front of a substance in a balanced reaction is a molar quantity known as a molar coefficient B. Law of Conservation of Mass - Matter cannot be gained or lost in the process of a chemical reaction. The law of conservation of mass states that we must have a balanced equation. C. List five factors involved in the construction of an equation or "chemical recipe." 1. The identity of products and reactants must be specified. 2. Reactants are written to the left of the reaction arrow ( >) and products to the right. 3. The physical state of reactants and products is shown in parentheses; (s), (l), (g), and (aq) 4. The symbol over the reaction arrow mean that heat energy is necessary for the reaction to occur. 5. The equation must be balanced. Steps for balancing a chemical equation Step 1: Step 2: Step 3: Count the number of atoms of each element on both the product and reactant side. Determine which atoms are not balanced. Balance one atom at a time, using coefficients. Start with atoms that appear only once in the reactants and only once in the products. Usually leave Hydrogen atoms followed by Oxygen atoms until last. Step 4: After you believe that you have successfully balanced the equation, repeat Step 1, to be certain that mass conservation has been achieved. Note: DO NOT Change subscripts in a molecular formula (i.e., 2 NaCl X Na 2 Cl 2 ) 119

2 Double Displacement Reactions Demonstration Dr. Gergens - SD Mesa College Using the solubility rules for ionic salts (see your periodic table, front cover), predict whether mixing the two aqueous ionic salts (or aqueous strong acid) will produced an insoluble precipitate. CuSO4 (aq) NaNO3 (aq) HCl (aq) AgNO3 (aq) Na2CO3 (aq) CuSO4 (aq) all soluble all soluble Ag 2 SO 4 (s) CuCO 3 (s) NaNO3 (aq) all soluble all soluble all soluble HCl (aq) AgCl (s) H 2 O(l)+ CO 2 (g) AgNO3 (aq) Ag 2 CO 3 (s) Na2CO3 (aq) A. CuSO4 (aq) + NaNO3 (aq) No Reaction () B. CuSO4 (aq) + HCl (aq) C. 1 CuSO4 (aq) + 2 AgNO3 (aq) 1 Ag2 SO4 (s) + 1 Cu(NO3)2 (aq) D. CuSO4 (aq) + Na2CO3 (aq) E. NaNO3 (aq) + HCl (aq) F. 1 HCl (aq) + 1 AgNO3 (aq) 1 AgCl (s) + 1 NaNO 3 (aq) G. 2 HCl (aq) + 1 Na2CO3 (aq) 2 NaCl (aq) + 1 CO 2 (g) + 1 H 2 O(l) H. NaNO3 (aq) + AgNO3 (aq) I. NaNO3 (aq) + Na2CO3 (aq)

3 BALANCING PRACTICE Dr. Gergens - SD Mesa College a. Balance each of the following equations by adjusting the coefficients in front of the chemical formulas. b. List the physical state of each compound. c. Determine the driving force for each reaction. d. Classify each reaction in as many ways as possible. 1. Cu (s) + 2 AgNO 3 (aq) Cu(NO3 ) 2 (aq) + 2 Ag (s) Transfer of Electrons 2. 2 Al (s) + 3 S (s) Al2 S 3 (s) Transfer of Electrons 3. Na 2 CO 3 (aq) + CaCl 2 (aq) CaCO3 (s) + 2 NaCl (aq) Precipitation of CaCO Fe (s) + 3 Cl 2 (g) 2 FeCl3 (s) Transfer of Electrons 5. 2 Na 3 PO 4 (aq) + 3 BaCl 2 (aq) Ba3 (PO 4 ) 2 (s) + 6 NaCl (aq) Precipitation of Ba 3 (PO 4 ) NaOH (aq) + CuSO 4 (aq) Na2 SO 4 (aq) + Cu(OH) 2 (s) Precipitation of Cu(OH) 2 7. Mg(OH) 2 (s) + H 2 SO 4 (aq) MgSO4 (aq) + 2 H 2 O (l) Water Formation Acid-Base Reaction 8. 2 Al (s) + 6 HCl (aq) 2 AlCl3 (aq) + 3 H 2 (g) Hydrogen Gas Formation 9. 3 Mg (s) + 2 H 3 PO 4 (aq) Mg3 (PO 4 ) 2 (s) + 3 H 2 (g) Mg 3 (PO 4 ) 2 ppt & H 2 Gas 10. Br 2 (l) + 2 CuI (aq) 2 CuBr (aq) + I 2 (s) Transfer of Electrons reduced oxidized Single Replacement NaOH (aq) + FeCl 3 (aq) 3 NaCl (aq) + Fe(OH) 3 (s) Precipitation of Fe(OH) KBr (aq) + Pb(NO 3 ) 2 (aq) > 2 KNO3 (aq) + PbBr 2 (s) Precipitation of PbBr AlCl 3 (aq) + 3 H 2 SO 4 (aq) Al2 (SO 4 ) 3 (s) + 6 HCl (aq) Precipitation of Al 2 (SO 4 ) Al 2 (SO 4 ) 3 (aq) + 3 BaCl 2 (aq) 3 BaSO4 (s) + 2 AlCl 3 (aq) Precipitation of BaSO Cd(NO 3 ) 2 (aq) + H 2 S (l) CdS (s) + 2 HNO 3 (aq) Precipitation of CdS 116

4 DOUBLE REPLACEMENT REACTIONS AND PREDICTIONS PRACTICE Dr. Gergens - Mesa College a. Complete and balance each of the following equations for double replacement reactions. b. List the physical state of each compound. c. Determine the driving force for each reaction. 1. NaCl (aq) + AgNO 3 (aq) NaNO3 (aq) + AgCl (s) Precipitation of AgCl 2. BaCl 2 (aq) + H 2 SO 4 (aq) BaSO4 (s) + 2 HCl (aq) Precipitation of BaSO 4 3. NaOH (aq) + HCl (aq) NaCl (aq) + H 2 O (l) Water Formation 4. Na 2 CO 3 (aq) + 2 HCl (aq) 2 NaCl (aq) + H 2 O (l) + CO 2 (g) Water & Gas 5. H 2 SO 4 (aq) + 2 NaOH (aq) 2 H2 O (l) + Na 2 SO 4 (aq) Water Formation 6. FeCl 3 (aq) + 3 KOH (aq) Fe(OH)3 (s) + 3 KCl (aq) Precipitation of Fe(OH) 3 7. Na 2 SO 3 (aq) + 2 HCl (aq) 2 NaCl (aq) + H 2 SO 3 (l) Special Strong to Weak Acid 8. K 2 CrO 4 (aq) + Pb(NO 3 ) 2 (aq) 2 KNO3 (aq) + PbCrO 4 (s) Precipitation of PbCrO 4 9. NaC 2 H 3 O 2 (aq) + HNO 3 (aq) HC2 H 3 O 2 (l) + NaNO 3 (aq) Special Strong to Weak Acid 10. NaOH (aq) + NH 4 Cl (aq) NaCl (aq) + NH 3 (g) + H 2 O (l) Water & Gas BiCl 3 (aq) + 3 H 2 S (l) Bi2 S 3 (s) + 6 HCl (aq) Precipitation of Bi 2 S K 2 C 2 O 4 (aq) + 2 HCl (aq) 2 KCl (aq) + H 2 C 2 O 4 (l) Special Strong to Weak Acid H 3 PO 4 (aq) + 3 Ca(OH) 2 (aq) 6 H2 O (l) + Ca 3 (PO 4 ) 2 (s) Water & ppt of Ca 3 (PO 4 ) (NH 4 ) 2 CO 3 (aq) + 2 HBr (aq) 2 NH4 Br (aq) + H 2 O (l) + CO 2 (g) Water & Gas 15. (NH 4 ) 2 CO 3 (aq) + CaCl 2 (aq) 2 NH4 Cl (aq) + CaCO 3 (s) Precipitation of CaCO 3 117

5 MORE BALANCING PRACTICE Dr. Gergens - Mesa College a. Balance each of the following equations by adjusting the coefficients in front of the chemical formulas. b. List the physical state of each compound. c. Determine the driving force for each reaction. d. Classify each reaction in as many ways as possible Mg (s) + O 2 (g) 2 MgO (s) Transfer of Electrons 2. 2 KClO 3 (s) 2 KCl (s) + 3 O 2 (g) Transfer of Electrons reduced Decomposition oxidized 3. 3 Fe (s) + 2 O 2 (g) Fe3 O 4 (s) Transfer of Electrons 4. Mg (s) + 2 HCl (aq) MgCl2 (aq) + H 2 (g) Transfer of Electrons 5. 2 Na (s) + 2 H 2 O (l) 2 NaOH (aq) + H 2 (g) Transfer of Electrons 6. 3 Fe (s) + 4 H 2 O (l) Fe3 O 4 (s) + 4 H 2 (g) Transfer of Electrons Beneath each word equation write the formula equation and balance it S (s) + O 2 (g) SO2 (g) Transfer of Electrons 8. Zn (s) + H 2 SO 4 (aq) ZnSO4 (aq) + H 2 (g) Transfer of Electrons 9. C (s) + O 2 (g) CO2 (g) Transfer of Electrons H 2 (g) + O 2 (g) 2 H2 O (l) Transfer of Electrons Al (s) + 6 HCl (aq) 2 AlCl3 (aq) + 3 H 2 (g) Transfer of Electrons K (s) + 2 H 2 O (l) 2 KOH (aq) + H 2 (g) Transfer of Electrons 13. NaHCO 3 (s) + HC 2 H 3 O 2 (aq) > NaC2 H 3 O 2 (aq) + H 2 O (l) + CO 2 (g) You can try this chemical reaction at home! NO transfer of electrons 118

6 2. 2 AgNO 3 (aq) + CaBr 2 (aq) > 2 AgBr (s) + Ca(NO 3 ) 2 (aq) a. 2 Ag + (aq) + 2 NO Ca 2+ (aq) + 2 Br > 2 AgBr (s) + Ca 2+ (aq) + NO 3 b. Ag + (aq) + Br > AgBr (s) 3. NaCN (aq) + HCl (aq) > NaCl (aq) + HCN (g,aq) a. Na + (aq) + CN + H + (aq) + Cl > Na + (aq) + Cl + HCN (g,aq) b. H + (aq) + CN > HCN (g,aq) 4. AgCN (aq) + HCl (aq) > AgCl (s) + HCN (g,aq) a. Ag + (aq) + CN + H + (aq) + Cl > AgCl (s) + HCN (g,aq) b. Ag + (aq) + CN + H + (aq) + Cl > AgCl (s) + HCN (g,aq) 5. Ba(OH) 2 (aq) + Na 2 SO 4 (aq) > BaSO 4 (s) + 2 NaOH (aq) a. Ba 2+ (aq) + 2 OH + 2 Na + (aq) + SO > BaSO 4 (s) + 2 Na + (aq) + 2 OH b. Ba 2+ (aq) + SO > BaSO 4 (s) 6. Na 2 S (aq) + Hg(NO 3 ) 2 (aq) > 2 NaNO 3 (aq) + HgS (s) a. 2 Na + (aq) + S 2 + Hg 2+ (aq) + 2 NO > 2 Na + (aq) + 2 NO 3 + HgS (s) b. Hg 2+ (aq) + S > HgS (s) 7. ZnCl 2 (aq) + H 2 S (aq, g) > ZnS (s) + 2 HCl (aq) a. Zn 2+ (aq) + 2 Cl + 2 H + (aq) + S > ZnS (s) + 2 H + (aq) + 2 Cl b. Zn 2+ (aq) + S > ZnS (s) 8. Na 2 S (aq) + 2 HCl (aq) > 2 NaCl (aq) + H 2 S (aq, g) a. 2 Na + (aq) + S H + (aq) + 2 Cl > 2 Na + (aq) + 2 Cl + H 2 S (aq, g) b. 2 H + (aq) + S > H 2 S (aq, g) 9. 2 KC 2 H 3 O 2 (aq) + H 2 SO 4 (aq) > K 2 SO 4 (aq) + 2 HC 2 H 3 O 2 (l) a. 2 K + (aq) + 2 C 2 H 3 O H + (aq) + SO > 2 K + (aq) + SO HC 2 H 3 O 2 (l) b. H + (aq) + C 2 H 3 O > HC 2 H 3 O 2 (l)

7 10. HC 2 H 3 O 2 (l) + KOH (aq) > H 2 O (l) + KC 2 H 3 O 2 (aq) a. HC 2 H 3 O 2 (l) + K + (aq) + OH > H 2 O (l) + K + (aq) + C 2 H 3 O 2 b. C 2 H 3 O 2 (l) + OH > H 2 O (l) + C 2 H 3 O NH 4 OH (aq) + HCl (aq) > NH 4 Cl (aq) + H 2 O (l) a. NH 4 + (aq) + OH + H + (aq) + Cl > NH 4 + (aq) + Cl + H 2 O (l) b. H + (aq) + OH > H 2 O (l) NH 4 OH (aq) + FeCl 3 (aq) > 3 NH 4 Cl (aq) + Fe(OH) 3 (s) a. 3 NH 4 + (aq) + 3 OH + Fe 3+ (aq) + 3 Cl > 3 NH 4 + (aq) + 3 Cl + Fe(OH) 3 (s) b. Fe 3+ (aq) + 3 OH > Fe(OH) 3 (s) HNO 3 (aq) + Ca(OH) 2 (aq) > 2 H 2 O (l) + Ca(NO 3 ) 2 (aq) a. 2 H + (aq) + 2 NO 3 + Ca 2+ (aq) + 2 OH > 2 H 2 O (l) + Ca 2+ (aq) + 2 NO 3 b. H + (aq) + OH > H 2 O (l) AgNO 3 (aq) + Na 2 S (aq) > Ag 2 S (s) + 2 NaNO 3 (aq) a. 2 Ag + (aq) + 2 NO Na + (aq) + S > Ag 2 S (s) + 2 Na + (aq) + 2 NO 3 b. Ag + (aq) + S > Ag 2 S (s) 15. Cu(CN) 2 (aq) + 2 HCl (aq) > CuCl 2 (aq) + 2 HCN (g,aq) a. Cu 2+ (aq) + 2 CN + 2 H + (aq) + 2 Cl > Cu 2+ (aq) + 2 Cl + 2 HCN (g,aq) b. H + (aq) + CN > HCN (g,aq) Pb(NO 3 ) 2 (aq) + 2 AlCl 3 (aq) > 3 PbCl 2 (s) + 2 Al(NO 3 ) 3 (aq) a. 3 Pb 2+ (aq) + 6 NO Al 3+ (aq) + 6 Cl > 3 PbCl 2 (s) + 2 Al 3+ (aq) + 6 NO 3 b. Pb 2+ (aq) + 2 Cl > PbCl 2 (s) AgC 2 H 3 O 2 (aq) + MgSO 4 (aq) > Ag 2 SO 4 (s) + Mg(C 2 H 3 O 2 ) 2 (aq) a. 2 Ag + (aq) + 2 C 2 H 3 O 2 + Mg 2+ (aq) + SO > Ag 2 SO 4 (s) + Mg 2+ (aq) + 2 C 2 H 3 O 2 b. 2 Ag + (aq) + SO > Ag 2 SO 4 (s)

8 18. HC 2 H 3 O 2 (l) + NH 4 OH (aq) > H 2 O (l) + NH 4 C 2 H 3 O 2 (aq) a. HC 2 H 3 O 2 (l) + NH 4 + (aq) + OH > H 2 O (l) + NH 4 + (aq) + C 2 H 3 O 2 b. HC 2 H 3 O 2 (l) + OH > H 2 O (l) + C 2 H 3 O Fe(NO 3 ) 3 (aq) + K 3 PO 4 (aq) > FePO 4 (s) + 3 KNO 3 (aq) a. Fe 3+ (aq) + 3 NO K + (aq) + PO > FePO 4 (s) + 3 K + (aq) + 3 NO 3 b. Fe 3+ (aq) + PO > FePO 4 (s) 20. Na 2 CO 3 (aq) + H 2 SO 4 (aq) > Na 2 SO 4 (aq) + H 2 O (l) + CO 2 (g) a. 2 Na + (aq) + CO H + (aq) + SO > 2 Na + (aq) + SO H 2 O (l) + CO 2 (g) b. 2 H + (aq) + CO > H 2 O (l) + CO 2 (g) 21. Cu(NO 3 ) 2 (aq) + 2 NaOH (aq) > Cu(OH) 2 (s) + 2 NaNO 3 (aq) a. Cu 2+ (aq) + 2 NO Na + (aq) + 2 OH > Cu(OH) 2 (s) + 2 Na + (aq) + 2 NO 3 b. Cu 2+ (aq) + 2 OH > Cu(OH) 2 (s) Explain why each of the following mixing of reactants affords no reaction,. 22. NaNO 3 (aq) + HCl (aq) > Both products are soluble 23. Pb(NO 3 ) 2 (aq) + Hg(NO 3 ) 2 (aq) > Both products are reactants 24. CsCl (aq) + (NH 4 ) 2 SO 4 (aq) > Both products are soluble 25. K 2 SO 4 (aq) + NaClO 4 (aq) > Both products are soluble

Reaction Type & Balancing Review Questions

Reaction Type & Balancing Review Questions Reaction Type & Balancing Review Questions There are 20 questions sets in this review. The corresponding answers can be found in the second half of this document. 1. Match the term with its proper description.

More information

What physical evidence do we have that sodium hydroxide dissociates into ions when it dissolves in water? NaOH(s) Na + + OH -

What physical evidence do we have that sodium hydroxide dissociates into ions when it dissolves in water? NaOH(s) Na + + OH - Chemistry Date Period Name CW double replacement reactions 030812.doc Double Replacement Reactions Double replacement reactions are some of the most common reactions that are performed in the laboratory.

More information

Chemical Equations. What is a chemical equation? How do you balance a chemical equation? How do you identify the type of chemical equation?

Chemical Equations. What is a chemical equation? How do you balance a chemical equation? How do you identify the type of chemical equation? Chemical Equations What is a chemical equation? How do you balance a chemical equation? How do you identify the type of chemical equation? Chemical Equations A chemical equation is written as an expression

More information

Tutorial 5 NET IONIC EQUATIONS

Tutorial 5 NET IONIC EQUATIONS T-33 Tutorial 5 NET IONIC EQUATIONS The efficiency and extent of a chemical reaction is very much dependent upon the physical state (solid, liquid, gas, or solution) of reactants and products. Not surprisingly,

More information

Easy Examples: Hd 10 + Bu 8 HdBu. Introduction. (l) or (aq)? Introduction. Symbols. Yields or Produces. Balancing. (l) or (aq)?

Easy Examples: Hd 10 + Bu 8 HdBu. Introduction. (l) or (aq)? Introduction. Symbols. Yields or Produces. Balancing. (l) or (aq)? Chemical Equations Chemical Equations Like a recipe: Introduction Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) Symbols (s) (l) (aq) (g) Introduction Yields or Produces solid liquid aqueous gas (l) or

More information

The formation of a gas is evidence of. 1. A chemical change. 2. A physical change. 3. No change in energy 4. Both (1) and (2)

The formation of a gas is evidence of. 1. A chemical change. 2. A physical change. 3. No change in energy 4. Both (1) and (2) Chapter 8 Review The formation of a gas is evidence of 1. A chemical change. 2. A physical change. 3. No change in energy 4. Both (1) and (2) The formation of a gas is evidence of 1. A chemical change.

More information

Types of Chemical Reactions

Types of Chemical Reactions Why? Types of Chemical Reactions Do atoms rearrange in predictable patterns during chemical reactions? Recognizing patterns allows us to predict future behavior. Weather experts use patterns to predict

More information

Do Now CHEMICAL REACTIONS. Chemical Reaction. chemical reaction. Chemical Equations. Evidence

Do Now CHEMICAL REACTIONS. Chemical Reaction. chemical reaction. Chemical Equations. Evidence Do Now CHEMICAL REACTIONS What are some signs that a chemical change may have taken place? Where are the reactants and products in a reaction? What do they represent? Describe the law of conservation of

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written

More information

Ch. 9 Chemical Reactions

Ch. 9 Chemical Reactions Ch. 9 Chemical Reactions I. Intro to Reactions (p. 282 285) I II III IV V Chemical Reaction Chemical change Atoms of one or more substances (reactants) are rearranged into new substances (products) Signs

More information

CHEMICAL REACTIONS. When sodium bicarbonate, e.g. baking soda, is combined with an acid, a gas is produced

CHEMICAL REACTIONS. When sodium bicarbonate, e.g. baking soda, is combined with an acid, a gas is produced CHEMICAL REACTIONS OBJECTIVES 1. To study reactions between ions in aqueous solutions 2. To observe exothermic and endothermic reactions 3. To study oxidation-reduction reactions 4. To practice balancing

More information

CHM1 Review for Exam 9

CHM1 Review for Exam 9 Topics 1. Reaction Types a. Combustion b. Synthesis c. Decomposition d. Single replacement i. Metal activity series ii. Nonmetal activity series e. Double replacement i. Precipitates and solubility rules

More information

Ch 8 Notes: Chemical Equations and Reactions

Ch 8 Notes: Chemical Equations and Reactions Name: Ch 8 Notes: Chemical Equations and Reactions I. Chemical Equations A properly written chemical equation can summarize any chemical change. The following requirements will help you write and read

More information

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure

More information

NET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is:

NET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NET IONIC EQUATIONS A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NaCl + AgNO 3 AgCl + NaNO 3 In this case, the simple formulas of the various reactants

More information

2. DECOMPOSITION REACTION ( A couple have a heated argument and break up )

2. DECOMPOSITION REACTION ( A couple have a heated argument and break up ) TYPES OF CHEMICAL REACTIONS Most reactions can be classified into one of five categories by examining the types of reactants and products involved in the reaction. Knowing the types of reactions can help

More information

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction Introduction Chapter 5 Chemical Reactions and Equations Chemical reactions occur all around us. How do we make sense of these changes? What patterns can we find? 1 2 Copyright The McGraw-Hill Companies,

More information

Net Ionic Equations Making Sense of Chemical Reactions

Net Ionic Equations Making Sense of Chemical Reactions 14 Making Sense of Chemical Reactions OBJECTIVE Students will be able to write net ionic equations from balanced molecular equations. LEVEL Chemistry NATIONAL STANDARDS UCP.1, UCP.2, B.3 T E A C H E R

More information

Chemical Reactions and Equations. Chapter 8

Chemical Reactions and Equations. Chapter 8 Chemical Reactions and Equations Chapter 8 Describing Chemical Reactions A chemical reaction is the process by which one or more substances are changed into different substances Reactants Products When

More information

Chapter 5 Chemical Reactions and Equations

Chapter 5 Chemical Reactions and Equations Chapter 5 Chemical Reactions and Equations 5.1 (a) single-displacement reaction; (b) anhydrous; (c) molecular equation; (d) decomposition reaction; (e) balanced equation; (f) reactant; (g) spectator ion;

More information

Chapter 8: Chemical Equations and Reactions

Chapter 8: Chemical Equations and Reactions Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical

More information

Chemical reactions. Classifications Reactions in solution Ionic equations

Chemical reactions. Classifications Reactions in solution Ionic equations Chemical reactions Classifications Reactions in solution Ionic equations Learning objectives Distinguish between chemical and physical change Write and balance chemical equations Describe concepts of oxidation

More information

CHAPTER 9 CALCULATIONS FROM CHEMICAL EQUATIONS SOLUTIONS TO REVIEW QUESTIONS. = 2 mol PH 3. a g b = 0.4 g PH. = 12 mol H 2 O.

CHAPTER 9 CALCULATIONS FROM CHEMICAL EQUATIONS SOLUTIONS TO REVIEW QUESTIONS. = 2 mol PH 3. a g b = 0.4 g PH. = 12 mol H 2 O. HEINS09-095-117v4.qxd 1/30/06 1:58 PM Page 95 CHAPTER 9 CALCULATIONS FROM CHEMICAL EQUATIONS SOLUTIONS TO REVIEW QUESTIONS 1. A e ratio is the ratio between the e amounts of two atoms and/or ecules involved

More information

Student Exploration: Chemical Equations

Student Exploration: Chemical Equations Name: Date: Student Exploration: Chemical Equations Vocabulary: Avogadro s number, chemical equation, chemical formula, chemical reaction, coefficient, combination, combustion, conservation of matter,

More information

13 Chemical Reactions

13 Chemical Reactions www.ck12.org 275 CHAPTER 13 Chemical Reactions CHAPTER OUTLINE 13.1 CHEMICAL REACTIONS AND EQUATIONS 13.2 BALANCING CHEMICAL EQUATIONS 13.3 TYPES OF REACTIONS CHAPTER 13. CHEMICAL REACTIONS 276 www.ck12.org

More information

What is a chemical reaction?

What is a chemical reaction? Chapter 5 Chemical Reactions and Equations What is a chemical reaction? How do we know a chemical reaction occurs? Writing chemical equations Predicting chemical reactions Representing reactions in aqueous

More information

CP Chapter 11 Notes Reactions and Equations

CP Chapter 11 Notes Reactions and Equations CP Chapter 11 Notes Reactions and Equations Evidence of Chemical Reactions How can you tell a reaction has taken place? Temperature change Color change Gas/bubbles Appearance of a (precipitate) Chemical

More information

Chapter 9. Answers to Questions

Chapter 9. Answers to Questions Chapter 9 Answers to Questions 1. Word equation: Silicon Tetrachloride + Water Silicon Dioxide + Hydrogen Chloride Formulas: Next, the chemical formulas are needed. As these are all covalent compounds,

More information

Experiment 1 Chemical Reactions and Net Ionic Equations

Experiment 1 Chemical Reactions and Net Ionic Equations Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical

More information

Chapter 6 Notes Science 10 Name:

Chapter 6 Notes Science 10 Name: 6.1 Types of Chemical Reactions a) Synthesis (A + B AB) Synthesis reactions are also known as reactions. When this occurs two or more reactants (usually elements) join to form a. A + B AB, where A and

More information

AP Chem Unit 1 Assignment 3 Chemical Equations

AP Chem Unit 1 Assignment 3 Chemical Equations Symbols used in chemical equations: Symbol Meaning + used to separate one reactant or product from another used to separate the reactants from the products - it is pronounced "yields" or "produces" when

More information

Chapter 8 Review and Study Guide

Chapter 8 Review and Study Guide Name: Class: Date: Chapter 8 Review and Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Knowledge about what products are produced in a chemical

More information

GHW#9. Louisiana Tech University, Chemistry 100. POGIL Exercise on Chapter 4. Quantities of Reactants and Products: Equations, Patterns and Balancing

GHW#9. Louisiana Tech University, Chemistry 100. POGIL Exercise on Chapter 4. Quantities of Reactants and Products: Equations, Patterns and Balancing GHW#9. Louisiana Tech University, Chemistry 100. POGIL Exercise on Chapter 4. Quantities of Reactants and Products: Equations, Patterns and Balancing Why? In chemistry, chemical equations represent changes

More information

QUALITATIVE ANALYSIS

QUALITATIVE ANALYSIS QUALITATIVE ANALYSIS Objectives: 1. To perform spot test precipitation reactions. 2. To write and balance precipitation reaction equations. 3. To learn how to balance equations. 4. To learn the solubility

More information

Reactions in Aqueous Solution

Reactions in Aqueous Solution CHAPTER 7 1. Water is the most universal of all liquids. Water has a relatively large heat capacity and a relatively large liquid range, which means it can absorb the heat liberated by many reactions while

More information

Balancing Chemical Equations Worksheet

Balancing Chemical Equations Worksheet Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.

More information

6 Reactions in Aqueous Solutions

6 Reactions in Aqueous Solutions 6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface

More information

Chapter 7: Chemical Equations. Name: Date: Period:

Chapter 7: Chemical Equations. Name: Date: Period: Chapter 7: Chemical Equations Name: Date: Period: 7-1 What is a chemical reaction? Read pages 232-237 a) Explain what a chemical reaction is. b) Distinguish between evidence that suggests a chemical reaction

More information

David A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College

David A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,

More information

Writing, Balancing and Predicting Products of Chemical Reactions.

Writing, Balancing and Predicting Products of Chemical Reactions. Writing, Balancing and Predicting Products of Chemical Reactions. A chemical equation is a concise shorthand expression which represents the relative amount of reactants and products involved in a chemical

More information

1. Sb + Cl 2 SbCl Mg + O 2 MgO _. 3. CaCl 2 Ca + Cl NaClO 3 NaCl + O Fe + HCl FeCl 2 + H CuO + H 2 Cu + H 2 O

1. Sb + Cl 2 SbCl Mg + O 2 MgO _. 3. CaCl 2 Ca + Cl NaClO 3 NaCl + O Fe + HCl FeCl 2 + H CuO + H 2 Cu + H 2 O Year 11 Chemistry Balancing Equations 1. Sb + Cl 2 SbCl 3 2. Mg + O 2 MgO _ 3. CaCl 2 Ca + Cl 2 4. NaClO 3 NaCl + O 2 5. Fe + HCl FeCl 2 + H 2 6. CuO + H 2 Cu + H 2 O 7. Al + H 2 SO 4 Al 2 (SO 4 ) 3 +

More information

Reduction. The gain of electron(s), causing the oxidation number of a species to

Reduction. The gain of electron(s), causing the oxidation number of a species to Reactions Word Coefficient Decomposition Double replacement Law of conservation of charge Law of conservation of energy Law of conservation of mass Mole ratio Oxidation Precipitate Product Reactant Reaction

More information

CHEMISTRY COMPUTING FORMULA MASS WORKSHEET

CHEMISTRY COMPUTING FORMULA MASS WORKSHEET CHEMISTRY COMPUTING FORMULA MASS WORKSHEET Directions: Find the formula mass of the following compounds. Round atomic masses to the tenth of a decimal place. Place your final answer in the FORMULA MASS

More information

Answers and Solutions to Text Problems

Answers and Solutions to Text Problems Chapter 6 Answers and Solutions 6 Answers and Solutions to Text Problems 6.1 A chemical change occurs when the atoms of the initial substances rearrange to form new substances. Chemical change is indicated

More information

c. PCl 3 (l) + 3H 2 O(l) H 3 PO 3 (l) + 3HCl(g)

c. PCl 3 (l) + 3H 2 O(l) H 3 PO 3 (l) + 3HCl(g) Chapter 9 Chemical Quantities 1. Although we define mass as the amount of matter in a substance, the units in which we measure mass are a human invention. Atoms and molecules react on an individual particleby-particle

More information

Stoichiometry Review

Stoichiometry Review Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen

More information

Equation Writing. CO 2 + H 2 O H 2 CO 3 reactants products

Equation Writing. CO 2 + H 2 O H 2 CO 3 reactants products Equation Writing A chemical equation is a concise shorthand expression which represents the relative amount of reactants and products involved in a chemical reaction. CO 2 + H 2 O H 2 CO 3 reactants products

More information

Potassium + Chlorine. K(s) + Cl 2 (g) 2 KCl(s)

Potassium + Chlorine. K(s) + Cl 2 (g) 2 KCl(s) Types of Reactions Consider for a moment the number of possible chemical reactions. Because there are millions of chemical compounds, it is logical to expect that there are millions of possible chemical

More information

Chapter 7 Chemical Reactions. Chemical & Physical Changes

Chapter 7 Chemical Reactions. Chemical & Physical Changes Chapter 7 Chemical Reactions Chemical & Physical Changes In a physical change, the chemical composition of the substance remains constant. Examples of physical changes are the melting of ice or the boiling

More information

Reactions in solution. A subset of chemical reactions

Reactions in solution. A subset of chemical reactions Reactions in solution A subset of chemical reactions Learning objectives Define solution and its components Distinguish among strong, weak and non-electrolyte Identify strong acids and strong bases Apply

More information

AN INVESTIGATION OF CHEMICAL REACTIONS II PART I: RELATIVE REACTIVITIES PRE-LAB QUERIES

AN INVESTIGATION OF CHEMICAL REACTIONS II PART I: RELATIVE REACTIVITIES PRE-LAB QUERIES NAME PARTNER(S) SECTION DATE AN INVESTIGATION OF CHEMICAL REACTIONS II This activity explores the reactivity of a number of metals using single replacement reactions and investigates the role of solubility

More information

Chemical Reactions and Equations

Chemical Reactions and Equations Chemical Reactions and Equations Thousands of chemical reactions take place in nature, in industrial processes, and in laboratories. They are described by Chemical Equations. There are two sides to a chemical

More information

Solutions CHAPTER Specific answers depend on student choices.

Solutions CHAPTER Specific answers depend on student choices. CHAPTER 15 1. Specific answers depend on student choices.. A heterogeneous mixture does not have a uniform composition: the composition varies in different places within the mixture. Examples of non homogeneous

More information

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12

More information

1. Given the balanced equations representing two chemical reactions:

1. Given the balanced equations representing two chemical reactions: Name: 1. Given the balanced equations representing two chemical reactions: Cl2 + 2NaBr 2NaCl + Br 2 2NaCl 2Na + Cl2 Which type of chemical reactions are represented by these equations? A) single replacement

More information

STOICHOMETRY UNIT Determine the mass of carbon present in a sample of glucose weighing 5.4 g.

STOICHOMETRY UNIT Determine the mass of carbon present in a sample of glucose weighing 5.4 g. PERCENTAGE COMPOSITION STOICHOMETRY UNIT 3 1. A sample of magnesium weighing 2.246 g burns in oxygen to form 3.724 g of magnesium oxide. What are the percentages of magnesium and oxygen in magnesium oxide?

More information

Part I: Parts and Meaning of a Chemical Equation:

Part I: Parts and Meaning of a Chemical Equation: Chemical Equations Name: Period: Date: Part I: Parts and Meaning of a Chemical Equation: 1) = process by which one or more substances are changed into one or more different substances (atoms are rearranged)

More information

Name Date Class CHEMICAL REACTIONS. SECTION 8.1 DESCRIBING CHEMICAL CHANGE (pages )

Name Date Class CHEMICAL REACTIONS. SECTION 8.1 DESCRIBING CHEMICAL CHANGE (pages ) 8 CHEMICAL REACTIONS SECTION 8.1 DESCRIBING CHEMICAL CHANGE (pages 203 211) This section explains how to write equations describing chemical reactions using appropriate symbols. It also describes how to

More information

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation.

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation. CEMICAL REACTIONS 1 ydrogen + Oxygen Water 2 + O 2 2 O reactants product(s) reactant substance before chemical change product substance after chemical change Conservation of Mass During a chemical reaction,

More information

SOLUBILITY CURVES WORKSHEET

SOLUBILITY CURVES WORKSHEET SOLUBILITY CURVES WORKSHEET 1.) Which compound is least soluble at 20 o C? At 80 o C? 2.) Which substance is the most soluble at 10 o C? At 50 o C? At 90 o C? 3.) The solubility of which substance is most

More information

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions Chapter 4: Solution Stoichiometry Cont. 1 Aqueous Solutions Molarity (dilution calculations, solution stoichiometry); Solubility and Solubility Rules Molecular, Ionic and Net Ionic Equations Precipitation

More information

11.3 Reactions in Aqueous Essential Understanding Reactions that occur in aqueous solutions are double-replacement

11.3 Reactions in Aqueous Essential Understanding Reactions that occur in aqueous solutions are double-replacement 11.3 Reactions in Aqueous Solution Essential Understanding Reactions that occur in aqueous solutions are double-replacement reactions. The products are precipitates, water, or gases. Lesson Summary Net

More information

Solubility Rules and Net Ionic Equations

Solubility Rules and Net Ionic Equations Solubility Rules and Net Ionic Equations Why? Solubility of a salt depends upon the type of ions in the salt. Some salts are soluble in water and others are not. When two soluble salts are mixed together

More information

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g) 1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)

More information

Types of Chemical Reactions (rxns.)

Types of Chemical Reactions (rxns.) Types of Chemical Reactions (rxns.) Chemical reactions occur when bonds (between the electrons of atoms) are formed or broken Chemical reactions involve l changes in the chemical composition of matter

More information

Name Class Date. Chapter: Chemical Equations and Reactions

Name Class Date. Chapter: Chemical Equations and Reactions Assessment Chapter Test B Chapter: Chemical Equations and Reactions PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question

More information

AP Chemistry Unit 7- Homework Problems Equilibrium and K sp

AP Chemistry Unit 7- Homework Problems Equilibrium and K sp AP Chemistry Unit 7- Homework Problems Equilibrium and K sp Nature of the Equilibrium State 1. Draw on this graph where equilibrium has been reached. [X] equilibrium time 2. What are three qualities of

More information

Chapter 7: Chemical Reactions

Chapter 7: Chemical Reactions Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that

More information

Chemical Reactions 2 The Chemical Equation

Chemical Reactions 2 The Chemical Equation Chemical Reactions 2 The Chemical Equation INFORMATION Chemical equations are symbolic devices used to represent actual chemical reactions. The left side of the equation, called the reactants, is separated

More information

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an

More information

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions. Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration

More information

Identify the letter of the choice that best completes the statement or answers the question.

Identify the letter of the choice that best completes the statement or answers the question. Chemistry Test - Chapter 10 Chemical Equations Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. When balancing a chemical equation, insert

More information

Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ

Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical

More information

V. POLYPROTIC ACID IONIZATION. NOTICE: K a1 > K a2 > K a3 EQUILIBRIUM PART 2. A. Polyprotic acids are acids with two or more acidic hydrogens.

V. POLYPROTIC ACID IONIZATION. NOTICE: K a1 > K a2 > K a3 EQUILIBRIUM PART 2. A. Polyprotic acids are acids with two or more acidic hydrogens. EQUILIBRIUM PART 2 V. POLYPROTIC ACID IONIZATION A. Polyprotic acids are acids with two or more acidic hydrogens. monoprotic: HC 2 H 3 O 2, HCN, HNO 2, HNO 3 diprotic: H 2 SO 4, H 2 SO 3, H 2 S triprotic:

More information

Chemical Reactions Chapter 8 Assignment & Problem Set

Chemical Reactions Chapter 8 Assignment & Problem Set Chemical Reactions Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Reactions 2 Study Guide: Things You Must Know Vocabulary (know the

More information

Aqueous Ions and Reactions

Aqueous Ions and Reactions Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for

More information

Chemistry AS90171 Describe chemical reactions

Chemistry AS90171 Describe chemical reactions Chemistry AS90171 Describe chemical reactions This achievement standard involves the description of chemical reactions, including the carrying out of calculations. Achievement Merit Excellence Describe

More information

Test 4: Equations and Math of Equations Review

Test 4: Equations and Math of Equations Review Name: Tuesday, November 27, 2007 Test 4: Equations and Math of Equations Review 1. Given the balanced equation: 2KClO 2KCl + 3O 3 2 Which type of reaction is represented by this equation? 1. synthesis

More information

EXPERIMENT #12 DOUBLE-REPLACEMENT REACTIONS

EXPERIMENT #12 DOUBLE-REPLACEMENT REACTIONS EXPERIMENT #12 DOUBLE-REPLACEMENT REACTIONS Purpose: 1. To study the most common type of double-replacement reactions. Principles: In double-replacement reactions, two compounds are involved in a reaction,

More information

Chapter 4: Reactions in Aqueous Solution (Sections )

Chapter 4: Reactions in Aqueous Solution (Sections ) Chapter 4: Reactions in Aqueous Solution (Sections 4.1-4.12) Chapter Goals Be able to: Classify substances as electrolytes or nonelectrolytes. Write molecular, ionic, and net ionic equations for precipitation,

More information

Types of Chemical Reactions Pre-Lab Assignment

Types of Chemical Reactions Pre-Lab Assignment Types of Chemical Reactions Pre-Lab Assignment Name Period Date The pre-lab is due at the beginning of the laboratory period 1. Read the entire procedure before beginning this pre-lab assignment. What

More information

Steps to Predicting the Products of Chemical Reactions. CP Chemistry

Steps to Predicting the Products of Chemical Reactions. CP Chemistry Steps to Predicting the Products of Chemical Reactions CP Chemistry TYPES OF REACTIONS REVIEW 2 NaNO 3 + PbO Pb(NO 3 ) 2 + Na 2 O C 2 H 4 O 2 + 2 O 2 2 CO 2 + 2 H 2 O ZnSO 4 + Li 2 CO 3 ZnCO 3 + Li 2 SO

More information

Laboratory 6: Double Displacement Reactions

Laboratory 6: Double Displacement Reactions Introduction Double displacement reactions are among the most common of the simple chemical reactions to study and understand. We will explore the driving forces behind the chemical reactions, and use

More information

Balancing Chemical Equations

Balancing Chemical Equations Balancing Chemical Equations 1. sodium carbonate + calcium hydroxide sodium hydroxide + calcium carbonate Na 2 CO 3 + Ca(OH) 2 2 NaOH + CaCO 3 2. carbon dioxide + water carbonic acid CO 2 + H 2 O H 2 CO

More information

Experiment 5: Studying Chemical Reactions

Experiment 5: Studying Chemical Reactions 1 Experiment 5: Studying Chemical Reactions When a chemical reaction occurs, substances called reactants are transformed into different substances called products that may have different appearances and

More information

This is Chemical Reactions and Equations, chapter 4 from the book Beginning Chemistry (index.html) (v. 1.0).

This is Chemical Reactions and Equations, chapter 4 from the book Beginning Chemistry (index.html) (v. 1.0). This is Chemical Reactions and Equations, chapter 4 from the book Beginning Chemistry (index.html) (v. 1.0). This book is licensed under a Creative Commons by-nc-sa 3.0 (http://creativecommons.org/licenses/by-nc-sa/

More information

Chemical Equations and Chemical Reactions. Chapter 8.1

Chemical Equations and Chemical Reactions. Chapter 8.1 Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.

More information

CHEM 110: CHAPTER 3: STOICHIOMETRY: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS

CHEM 110: CHAPTER 3: STOICHIOMETRY: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS 1 CHEM 110: CHAPTER 3: STOICHIOMETRY: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS The Chemical Equation A chemical equation concisely shows the initial (reactants) and final (products) results of

More information

Experiment 9 - Double Displacement Reactions

Experiment 9 - Double Displacement Reactions Experiment 9 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

More information

Answers to Practice Problems 6.1, p Answers to Practice Problems 6.2, p. 227

Answers to Practice Problems 6.1, p Answers to Practice Problems 6.2, p. 227 Answers to Practice Problems 6.1, p. 226 1. This is a synthesis reaction (between a metal and a non-metal). The balanced chemical equation is: 2Li + Cl 2 2LiCl. 2. This is a synthesis reaction (between

More information

Science 1194 SAS Curriculum Pathways Chemical Equations: Journal

Science 1194 SAS Curriculum Pathways Chemical Equations: Journal Chemical Equations: Journal NAME: ray CLASS: chem90 DATE: 10/27/2013 FOCUS QUESTION: How and why are chemical equations balanced? TAB 1: Equations Read the questions below. Then complete this Journal by

More information

Unit 8: Reactions. Student Name: Key. Class Period: _3, 5, & 10_. Unit 8: Reactions-Key Regents Chemistry Mr. Murdoch

Unit 8: Reactions. Student Name: Key. Class Period: _3, 5, & 10_. Unit 8: Reactions-Key Regents Chemistry Mr. Murdoch Unit 8: Reactions Student Name: Key Class Period: _3, 5, & 10_ Website upload 2015 Page 1 of 57 Lecture Key Page intentionally blank Website upload 2015 Page 2 of 57 Lecture Key Unit 8 Vocabulary: 1. Coefficient:

More information

CHEMICAL REACTIONS. Chemistry 51 Chapter 6

CHEMICAL REACTIONS. Chemistry 51 Chapter 6 CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,

More information

Classifying equations tutorial:

Classifying equations tutorial: Classifying equations tutorial: Students are required to classify 5 kinds of equations. Indicator C-4.1 Indicator C-4.1 in the South Carolina Science Standards students should be able to analyze and balance

More information

4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes

4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes Chapter 4 Reactions in Aqueous Solution 4.1 Aqueous Solutions Solution homogeneous mixture of 2 or more substances Solute the substance present in a smaller amount (usually solid in Chap. 4) Solvent the

More information

3. Which of the following describes a conjugate acid-base pair for the following equilibrium? CN - (aq) + CH 3 NH 3 + (aq) H 2 CO 3 (aq) + H 2 O (l)

3. Which of the following describes a conjugate acid-base pair for the following equilibrium? CN - (aq) + CH 3 NH 3 + (aq) H 2 CO 3 (aq) + H 2 O (l) Acids, Bases & Redox 1 Practice Problems for Assignment 8 1. A substance which produces OH ions in solution is a definition for which of the following? (a) an Arrhenius acid (b) an Arrhenius base (c) a

More information

Chapter 8 - Chemical Equations and Reactions

Chapter 8 - Chemical Equations and Reactions Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from

More information

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11 SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436

More information

Chapter 5 Chemical Quantities and Reactions

Chapter 5 Chemical Quantities and Reactions Chapter 5 Chemical Quantities and Reactions 1 Avogadro's Number Small particles such as atoms, molecules, and ions are counted using the mole. 1 mole = 6.02 x 10 23 items Avogadro s number 602 000 000

More information

Balancing Chemical Equations Worksheet Intermediate Level

Balancing Chemical Equations Worksheet Intermediate Level Balancing Chemical Equations Worksheet Intermediate Level Neutralization Reactions Salts are produced by the action of acids. Salts are written metal first, then non-metal. Eg. NaCl not ClNa Acid + Base

More information