Chapter 4: Stoichiometry of Chemical Reactions. 4.1 Writing and Balancing Chemical Equations
|
|
- Shanon Dickerson
- 5 years ago
- Views:
Transcription
1 Chapter 4: Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations A chemical equation represents or symbolizes a chemical reaction. o Substances are represents by their chemical formulas. o Relative amounts are indicated by numeric coefficients. The morphology or structure of a chemical equation: Note that an equation relates numbers of substances, not masses. Any number interpretation is valid: o Microscopic: equation gives the number of atoms and molecules. o Macroscopic: equation gives the number of moles of the substances. 1 Chem 180-Spring 2019
2 Stoichiometry requires a balanced chemical equation! o Dalton s Postulate: atoms are neither created nor destroyed in a chemical reaction (they are simply rearranged). o To balance a chemical equation, we need to achieve the same number and types of atoms on both sides of the equation, reactant & product. When given the reactants and products of a reaction, we may only change the coefficients to balance the equation! o Changing any of the chemical formulas changes the reaction. o The coefficients should be the smallest whole numbers that balance the equation. For now, the equations we balance are relatively simply and we can verify one is balanced by inspection: manually count the numbers of each element and see that the reactant numbers equal the product numbers. o Be sure to count atoms that appear in more than one formula. o A subscript only applies to the preceding element. o A subscript after a closing parenthesis applies to all the atoms inside the parentheses. o A coefficient applies to all the atoms following the coefficient. We can multiply coefficient by subscript to speed up our counting. o Note: If a formula is incorrect, you might not be able to balance! 2 Chem 180-Spring 2019
3 While balancing simple equations can involve some trial and error, systematic approaches can get the job done relatively quickly. o A balancing procedure might involve iteration (repetition) as balancing one element could unbalance another. o If you are rusty or unsure of yourself, the text s tabular approach helps organize the data. o I like to work from left to right balancing one element at a time. o Remember to keep polyatomic ions intact when balancing! count the N and O atoms on both sides change the coefficient of O on the left and recount change the coefficient of N on the left and recount Finished! (And always do one last recount to check!) 3 Chem 180-Spring 2019
4 N 2 + O 2 N 2 O 5 H 3 PO 4 + CaO Ca 3 (PO 4 ) 2 + H 2 O C 3 H 8 + O 2 CO 2 + H 2 O NO 2 + NH 3 N 2 + H 2 O Write and balance an equation for the combustion of thiosalicylic acid, C 7 H 6 O 2 S, used in the manufacture of indigo dyes. Start using state symbols in your equations: (s), (l), (g), (aq). You already know or can predict many of them. o All elemental metals except Hg are solid at room temperature (RT). o Elemental nonmetals are solids and gases, and one liquid, Br 2. o All ionic compounds are solid (b/c of strong ionic attractions). o Molecular compounds tend to be liquids, but light ones are gases. We may write reaction conditions above and below the arrow: 2 Ag 2 O(s) 4 Ag(s) + O 2 (g) 350 C CO(g) + 2 H 2 (g) CH 3 OH(g) 340 atm, ZnO, Cr 2 O 3 4 Chem 180-Spring 2019
5 When ionic reactants and products are involved, we can write three different equations to summarize the chemical changes taking place. o We see ionic equations a lot in lab! The three equations are: o Molecular (Formula): only uncharged compound formulas are shown. o Complete (Total) Ionic: (aq) strong electrolytes are dissociated. Strong electrolytes are soluble ionic compounds and strong acids. o Net Ionic: rewrite complete ionic and omit the spectator ions. Word eqn: When aqueous solutions of CaCl 2 and AgNO 3 are mixed, a reaction takes place producing aqueous Ca(NO 3 ) 2 and solid AgCl. Molecular Eqn: CaCl 2 (aq) + AgNO 3 (aq) Ca(NO 3 ) 2 (aq) + AgCl(s) CaCl 2 (aq) + 2 AgNO 3 (aq) Ca(NO 3 ) 2 (aq) + 2 AgCl(s) balanced! Complete Ionic Eqn: Ca 2+ (aq) + 2 Cl (aq) + 2 Ag + (aq) + 2 NO 3 (aq) Ca 2+ (aq) + 2 NO 3 (aq) + 2 AgCl(s) Net Ionic Eqn: 2 Cl (aq) + 2 Ag + (aq) 2 AgCl(s) Cl (aq) + Ag + (aq) AgCl(s) coefficients simplified! When carbon dioxide is dissolved in an aqueous solution of sodium hydroxide, the mixture reacts to yield aqueous sodium carbonate and liquid water. Write balanced molecular, complete ionic, and net ionic equations for this reaction. 5 Chem 180-Spring 2019
6 4.2 Classifying Chemical Reactions After studying the reactants and products of chemical reactions, chemists have found that many can be classified into one of several types: o Precipitation reaction: dissolved substances react to form solid product(s). o Acid-Base reaction: a hydrogen ion is transferred from one species to another. Also known as a Neutralization reaction. The hydrogen ion is transferred via a water molecule as the hydronium ion, H 3 O + (aq). o Oxidation-Reduction reaction: this will be examined later in the course. Several other classifications exist, but we will concentrate on these. Precipitation and acid-base reactions are two types of the doubledisplacement reaction in which two species swap their anions. o Generically, we can the double-displacement reaction as: AB + CD AD + BC o An example of the precipitation double-displacement reaction is: NaCl(aq) + AgNO 3 (aq) NaNO 3 (aq) + AgCl(s) o An example of the acid-base double-displacement reaction is: HCl(aq) + NaOH(aq) HOH(l) + NaCl(aq) In general, Acid + Base Water + Salt Given the reactants of a double displacement reaction; you should be able to: o Complete the Molecular Eqn (predict the products and their states), o Balance the Molecular Eqn, and o Write the balanced Complete Ionic and Net Ionic Eqns. Also identify the Spectator Ions. 6 Chem 180-Spring 2019
7 Precipitation Reactions Solubility rules are used to predict the states of the products, (aq) or (s). o You should use the following rules as they are provided with tests. o These rules are consistent with this in your text, although they are presented differently. Solubility guidelines for common ionic solids Follow these rules in the order listed. When you come to a rule that applies to your compound, STOP. Conflicts are thus avoided. 1. Salts of group 1 metal cations and the NH 4 + cation are soluble. 2. Nitrates, acetates, bicarbonates, chlorates, and perchlorates are soluble. 3. Chlorides, bromides, and iodides are soluble, except for those of silver, lead(ii), and mercury(i). 4. Sulfates are soluble, except for those of Ca 2+, Sr 2+, and Ba Carbonates, phosphates, sulfides, oxides, chromates, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca 2+, Sr 2+, and Ba 2+ are slightly soluble). 6. If Rules 1 6 do not apply, the salt is probably insoluble. The steps to writing the Molecular, Complete Ionic, and Net Ionic Eqns. o To complete the Molecular equation for the reaction, apply double displacement to predict the products, and use the solubility rules to predict product states. Then balance the equation. There should be no ionic species in this equation that is, show no charges. o Write the balanced Complete Ionic equation by re-writing the Molecular equation, but substitute the strong electrolytes (soluble salts and strong acids) with their ions in solution. Use H 3 O + not H + for the strong acids! Be careful with subscripts and coefficients! o Identify the Spectator Ions in the Complete Ionic equation. Write the balanced Net Ionic equation by re-writing the Ionic equation, but omit the spectator ions. 7 Chem 180-Spring 2019
8 Complete and write the balanced molecular, complete ionic, and net ionic equations for: K 3 PO 4 (aq) + FeBr 2 (aq) If no ppt is formed, indicate this by writing no reaction or NR in the molecular eqn: <reactants> No Reaction <reactants> NR Acid-Base Reactions An acid is a molecular substance that dissolves in and reacts with water to produce H 3 O + (aq) ions. We call this process ionization. (Note the distinction from soluble salts whose ions dissociate.) o Strong acids are 100% ionized in aqueous solution: 100% HBr(aq) + H 2 O(l) H 3 O + (aq) + Br (aq) 8 Chem 180-Spring 2019
9 o Weak acids are not completely ionized; their reaction with water is reversible. HOOC-COOH(aq) + H 2 O(l) H 3 O + (aq) + HOOC-COO (aq) A base is an ionic (most commonly for us) or molecular substance that produces OH (aq) ions in water. o Strong bases are soluble metal hydroxides which generate hydroxide ions by dissociation: 100% KOH(s) K + (aq) + OH (aq) o Weak bases are molecular compounds that dissolve in and react with water to produce hydroxide ions by reversible ionization: NH 3 (aq) + H 2 O(l) NH 4 + (aq) + OH (aq) You should know these common strong acids and strong bases: 9 Chem 180-Spring 2019
10 To complete and write the three balanced equations for acid-base reactions, we follow the same steps we used for precipitation reactions. However, instead of forming a ppt, we form water! o When predicting the products, use H + from the acid. o When writing the ionic equations for strong acids, use H 3 O +. We implicitly add water on the reactant side to form H 3 O +, so do not forget to add H 2 O on the product side to keep the eqn balanced. o Weak acids are shown as molecules, not ionized, as reactants. Write the balanced Molecular, Complete Ionic, and Net ionic eqns for this strong acid strong base neutralization reaction: HNO 3 (aq) + Ba(OH) 2 (aq) Write the balanced Molecular, Complete Ionic, and Net ionic eqns for this weak acid strong base neutralization reaction: CH 3 COOH(aq) + NaOH(aq) 10 Chem 180-Spring 2019
11 4.3 Reaction Stoichiometry Now things get interesting! Solving stoichiometric problems can be challenging. Just think of it as being given an opportunity to excel! Stoichiometry refers to the quantitative calculations involving the relative amounts of reactants and products in a chemical reaction. Relative amounts are determined by the coefficients from the balanced chemical equation for the reaction. The fundamental unit for such calculations is the mole. Typical steps in stoichiometry are outlined below. The red box shows that all calculations include mole conversion from one species in the reaction to another. If we are not given moles of A, we must first find the moles of A If we are not asked for moles of B, we must then convert moles of B to the requested units. 1 mol A MM of A Step 2 MM of B 1 mol B y mol B x mol A = 1 mol A N A x and y are coefficients from the equation N A 1 mol B 11 Chem 180-Spring 2019
12 Let s dive right in! Potassium chlorate decomposes to solid potassium chloride and oxygen gas when heated. How many moles of O 2 are produced from the decomposition of 1.76 moles of potassium chlorate? How many grams of magnesium nitride are produced by the reaction of 3.82 g Mg with an excess of N 2? How many mg of H 2 are produced when one drop (0.05 ml) of hydrochloric acid solution (1.14 g/ml, 28.0% HCl by mass) reacts with an excess of aluminum to produce hydrogen gas and aqueous aluminum chloride. 12 Chem 180-Spring 2019
13 How many milliliters of M AgNO 3 (aq) are required to react completely with 175 ml of M K 2 CrO 4 (aq)? What mass of Ag 2 CrO 4 (s) is formed? 4.4 Reaction Yields So far, our stoichiometry has looked at reactions in which the stoichiometric amounts of reactants are present, that is, the relative amounts specified by the coefficients in the equation. (Or we were told one reactant was in excess.) But often reactants are not present in stoichiometric amounts, and one reactant runs out before the other. This limits the amount of product(s) formed. 13 Chem 180-Spring 2019
14 H 2 (g) + Cl 2 (g) 2 HCl(g) Identifying and solving limiting reactant problems: o In limiting reactant problems, you are given quantities of both reactants. o Pick a product, and convert each reactant to this product (moles or mass); that is, solve two stoichiometric equations. o The reactant that forms the smaller amount of product is the limiting reactant. o Suggestion: use the amount of the limiting reactant for other equation stoichiometry g H 2 and 154 g O 2 are allowed to react forming liquid water. Which gas is the limiting reactant, and what mass of the excess reactant remains? 14 Chem 180-Spring 2019
15 How many grams of barium sulfate will be formed from g of barium nitrate and g of sodium sulfate? What mass of the excess reactant is left over? Ba(NO 3 ) 2 (aq) + Na 2 SO 4 (aq) BaSO 4 (s) + 2 NaNO 3 (aq) Percent yield (% yield) = (actual yield / theoretical yield) * 100% What is the percent yield if the reaction of 25.0 g P 4 with 91.5 g Cl 2 produces 104 g PCl 3? 15 Chem 180-Spring 2019
16 How many grams of hydrogen chloride can be produced from g of hydrogen and 50.0 g of chlorine? H 2 (g) + Cl 2 (g) 2 HCl(g) If the theoretical yield for a reaction is 72.3 g of CCl 4, and 65.0 g of carbon tetrachloride was actually obtained, calculate the percent yield. (See example 9.13 on page 188 of your text for the complete calculation.) A sample of an alloy of iron and aluminum has a mass of 2.05 g. When the allow reacts with hydrochloric acid, g of hydrogen gas are collected. What is the percent by mass of iron in the alloy? 16 Chem 180-Spring 2019
Chemical reactions describe processes involving chemical change
1.1 Chemical Reactions 1.2 Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into
More informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More informationChapter 5 Classification and Balancing of Chemical Reactions
Chapter 5 Classification and Balancing of Chemical Reactions 5.1 Chemical Equations Chemical equations describe chemical reactions. - As words: hydrogen plus oxygen combine to form water - As a chemical
More informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Topics General properties of aqueous solutions Precipitation reactions Acid base reactions Oxidation reduction reactions Concentration of solutions Aqueous reactions
More informationPart 01 - Notes: Reactions & Classification
Objectives: Identify, define, and explain: combination reaction, synthesis reaction, decomposition reaction, single replacement reaction, double replacement reaction, combustion reaction, rapid oxidation,
More informationEquation Writing for a Neutralization Reaction
Equation Writing for a Neutralization Reaction An Acid-Base reaction is also called a Neutralization reaction because the acid (generates H + or H 3 O + ) and base (generates OH ) properties of the reactants
More informationCh 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the
More informationChapter 4 Types of Chemical Reaction and Solution Stoichiometry
Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because
More informationA reaction in which a solid forms is called a precipitation reaction. Solid = precipitate
Chapter 7 Reactions in Aqueous Solutions 1 Section 7.1 Predicting Whether a Reaction Will Occur Four Driving Forces Favor Chemical Change 1. Formation of a solid 2. Formation of water 3. Transfer of electrons
More informationChapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill
Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component
More informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More informationChemical Reactions and Equations
Chemical Reactions and Equations 5-1 5.1 What is a Chemical Reaction? A chemical reaction is a chemical change. A chemical reaction occurs when one or more substances is converted into one or more new
More informationChapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.
Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the
More informationinsoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water
Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of
More informationChapter 4. Types of Chemical Reactions and Solution Stoichiometry
Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Table of Contents 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition
More informationGeneral Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
More informationChapter 4. Chemical Quantities and Aqueous Reactions
Lecture Presentation Chapter 4 Chemical Quantities and Aqueous Reactions Reaction Stoichiometry: How Much Carbon Dioxide? The balanced chemical equations for fossilfuel combustion reactions provide the
More informationCHEMICAL REACTIONS. Introduction. Chemical Equations
CHEMICAL REACTIONS Chemistry I Chapter 7 1 Chemical Equations Their Job: Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The
More informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More informationName CHEMISTRY / / Oxide Reactions & Net Ionic Reactions
Name CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are two
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More informationName HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions
Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are
More informationChapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file)
Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file) Section 3.1: Solubility Rules (For Ionic Compounds in Water) Section 3.1.1: Introduction Solubility
More information7/16/2012. Chapter Four: Like Dissolve Like. The Water Molecule. Ionic Compounds in Water. General Properties of Aqueous Solutions
General Properties of Aqueous Solutions Chapter Four: TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY A solution is a homogeneous mixture of two or more substances. A solution is made when one substance
More informationSI session Grue 207A
Chem 105 Wednesday 21 Sept 2011 1. Precipitation and Solubility 2. Solubility Rules 3. Precipitation reaction equations 4. Net ionic equations 5. OWL 6. Acids and bases SI session Grue 207A TR, 12:001:30
More informationReactions in Aqueous Solutions
Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can
More informationChapter 7 Chemical Reactions
Chapter 7 Chemical Reactions Evidence of Chemical Change Release or Absorption of Heat Color Change Emission of Light Formation of a Gas Formation of Solid Precipitate Tro's "Introductory 2 How Do We Represent
More informationWhat Do You Think? Investigate GOALS
Cool Chemistry Show Activity 4 Chemical Equations GOALS In this activity you will: Represent chemical changes using word equations and chemical equations. Distinguish between different classes of chemical
More informationPart One: Ions in Aqueous Solution
A. Electrolytes and Non-electrolytes. CHAPTER FOUR: CHEMICAL REACTIONS Part One: Ions in Aqueous Solution 1. Pure water does not conduct electric current appreciably. It is the ions dissolved in the water
More informationReaction Classes. Precipitation Reactions
Reaction Classes Precipitation: synthesis of an ionic solid a solid precipitate forms when aqueous solutions of certain ions are mixed AcidBase: proton transfer reactions acid donates a proton to a base,
More informationChapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
More informationChemical Reactions CHAPTER Reactions and Equations
CHAPTER 9 Chemical Reactions 9.1 Reactions and Equations The process by which atoms of one or more substances are rearranged to form different substances is called a chemical reaction. There are a number
More informationChem 1A Dr. White Fall Handout 4
Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular
More informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
More informationCh 100: Fundamentals for Chemistry
Ch 100: Fundamentals for Chemistry Chapter 8: Chemical Equations Lecture Notes Chemical Equations (Intro) 1. Chemical equations are used to symbolically describe chemical reactions 2. In a chemical equation
More informationAP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry
I. IUPAC Naming AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry For Ionic Compounds: Formula to Name: 1. Identify the cation (positive ion) by name, then identify the
More informationChapter 5. Chemical reactions
Chapter 5 Chemical reactions Chemical equations CaO(s) + CO 2 (g) CaCO 3 (s) + CO(g) Chemical equation - representation of a chemical reaction; uses the symbols of the elements and formulae of the compounds
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationNET IONIC REACTIONS in AQUEOUS SOLUTIONS AB + CD AD + CB
NET IONIC REACTIONS in AQUEOUS SOLUTIONS Double replacements are among the most common of the simple chemical reactions. Consider the hypothetical reaction: AB + CD AD + CB where AB exists as A + and B
More informationCHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total.
Name Exam No. F CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total. Multiple Choice. (20 questions, 3 points each = 60 points total) Mark the letter on the scantron form corresponding to the one best
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationCHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS
CHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS CHEMICAL REACTIONS Occurs when matter combines or breaks apart to produce new kinds of matter with different properties with a change in energy. EVIDENCE FOR
More informationCH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
More informationFe(s) + O2(g) Chapter 11 Chemical Reactions. Chemical Equations. Fe + O2. January 26, What is a chemical reaction?
Chapter 11 Chemical Reactions What is a chemical reaction? Chemical Reaction: process by which one or more substances are changed into one or more different substances. Indications of a chemical reaction
More informationCHEMICAL REACTIONS. The process by which one or more substances are changed into one or more different substances
CHEMICAL REACTIONS The process by which one or more substances are changed into one or more different substances Equations Reactions are represented by a chemical equation Reactants Products Must have
More information9/24/12. Chemistry Second Edition Julia Burdge. Reactions in Aqueous Solutions
Chemistry Second Edition Julia Burdge 4 Reactions in Aqueous Solutions Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 4 Reactions in Aqueous Solutions
More informationChapter 9. Vocabulary Ch Kick Off Activity. Objectives. Interpreting Formulas. Interpreting Formulas
Chapter 9 Chemical Vocabulary Ch. 9.1 Chemical reaction Reactant Product Word Equation Skeleton Equation Chemical equation Coefficient 1 2 Objectives Write chemical equations to describe chemical reactions
More informationChemical Equations. Chemical Reactions. The Hindenburg Reaction 5/25/11
Chemical Reactions CHM 1032C Chemical Equations Chemical change involves a reorganization of the atoms in one or more substances. The Hindenburg Reaction Reactants are on left, products to the right. Arrow
More informationSolutions 4a (Chapter 4 problems)
Solutions 4a (Chapter 4 problems) Chem151 [Kua] 4.10 A balanced chemical equation must have equal numbers of atoms of each element on each side of the arrow. Balance each element in turn, beginning with
More informationSession 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67)
Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) I. Elecrolytes a. Soluble substances b. Insoluble substances c. Electrolytes d. Non-Electrolytes e. Ions and electrical conductivity f. Strong and
More informationUnit IV: Chemical Equations & Stoichiometry
Unit IV: Chemical Equations & Stoichiometry A. The chemical equation B. Types of chemical reactions A. Activity series of metals B. Solubility rules C. Rules for writing and balancing equations D. Calculations
More informationUNIT (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. Atomic mass
More informationIntro to Reactions/ Balancing Equations
Intro to Reactions/ Balancing Equations Chemical Reactions Chemical reactions involve change. Evidence of a chemical reaction could include the following Evolution of heat, light, and/or sound Production
More informationCh. 8 Chemical Reactions
Ch. 8 Chemical Reactions Intro to Reactions I II III IV V Signs of a Chemical Reaction Evolution of heat and light Formation of a gas Formation of a precipitate Color change Law of Conservation of Mass
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions
More informationNet Ionic Equations. Making Sense of Chemical Reactions
Making Sense of Chemical Reactions Now that you have mastered writing balanced chemical equations it is time to take a deeper look at what is really taking place chemically in each reaction. There are
More informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More informationChapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions
Chapter 4; Reactions in Aqueous Solutions I. Electrolytes vs. NonElectrolytes II. Precipitation Reaction a) Solubility Rules III. Reactions of Acids a) Neutralization b) Acid and Carbonate c) Acid and
More informationUnit 1 - Foundations of Chemistry
Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its
More informationChapter 4 Chemical Formulas, Reactions, Redox and Solutions
Terms to Know: Solubility Solute Solvent Solution Chapter 4 the amount of substance that dissolves in a given volume of solvent at a given temperature. a substance dissolved in a liquid to form a solution
More informationChapter 4. Reactions in Aqueous Solution. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 4 in Solution 2012 Pearson Education, Inc. John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Solutions Solute: substance in lesser quantity in
More informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
More informationCHM 130LL: Double Replacement Reactions
CHM 130LL: Double Replacement Reactions One of the main purposes of chemistry is to transform one set of chemicals (the reactants) into another set of chemicals (the products) via a chemical reaction:
More informationIONIC CHARGES. Chemistry 51 Review
IONIC CHARGES The ionic charge of an ion is dependent on the number of electrons lost or gained to attain a noble gas configuration. For most main group elements, the ionic charges can be determined from
More informationTypes of Reactions. There are five main types of chemical reactions we will talk about:
Chemical Reactions Types of Reactions There are five main types of chemical reactions we will talk about: 1. Synthesis reactions 2. Decomposition reactions 3. Single displacement reactions 4. Double displacement
More informationChemical Equations and Chemical Reactions
Chemical Equations Chemical Equations and Chemical Reactions Chemical equations are concise representations of chemical reactions. Chemical Equations Symbols Used in Chemical Equations The formulas of
More informationThe photograph in the textbook provides evidence that an exothermic chemical reaction is occurring.
Preview Lesson Starter Objectives Indications of a Chemical Reaction Characteristics of Chemical Equations Significance of a Chemical Equation Balancing Chemical Equations Section 1 Describing Chemical
More informationLaw of conservation of mass: Chemical reaction: conversion of substances into different substances (by rearranging atoms) H 2 + O 2 H 2 O
Chapter 7: Chemical Reactions Chemical reaction: conversion of substances into different substances (by rearranging atoms) Reactants: substances present before reaction Products: substances present after
More informationSolution Chemistry. Chapter 4
Solution Chemistry Chapter 4 Covalent Molecule Dissolving in Water Ionic Compound Dissolving in Water Electrolytes and Nonelectrolytes Electrolytes/Nonelectrolytes Type Dissociation Electrical Conductivity
More informationChemical Reaction Types
Chemical Reactions Chemical Reaction Types There are 5 types of chemical reactions that you need to know Combination reaction Decomposition reaction Combustion reaction Single replacement (redox) reaction
More informationLast Lecture. K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) AgNO 3 (aq) + KCl(aq) NaNO 3 (aq) + KCl(aq) What will happen when these are mixed together?
Announcements Precipitation lab write-up due tomorrow at the start of discussion Text HW due tomorrow in discussion Lon-capa HW #4 Type 1 due Monday, Oct 15 th at 7:00pm Lon-capa HW #4 Type 2 due Wednesday,
More informationAqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).
Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are
More informationI. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in Solution*
Chapter 5 Reactions in Aqueous Solutions Titrations Kick Acid!!! 1 I. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in
More informationTypes of Chemical Reactions (rxns.)
Types of Chemical Reactions (rxns.) Introduction Chemical reactions occur when bonds (between the electrons of atoms) are formed or broken Chemical reactions involve changes in the chemical composition
More informationYou try: 2) HC 7H 6O 2 3) N 2O 5. 5) HClO 4. 7) Rb 2C 2O 4 8) H 3PO 4 9) AgI 10) Sr(OH) 2. What kind of compound is it? NON ELECTROLYTE (NE)
Solubility: Solubility is the measure of how much of a solute will dissolve in a solvent. In general chemistry, we usually talk about water as the solvent, so we are talking about what compounds will dissolve
More informationChapter Four: Reactions in Aqueous Solution
Chapter Four: Reactions in Aqueous Solution Learning Outcomes: Identify compounds as acids or bases, and as strong, weak, or nonelectrolytes Recognize reactions by type and be able to predict the products
More informationChemical Change. Section 9.1. Chapter 9. Electrolytes and Solution Conductivity. Goal 1. Electrical Conductivity
Chapter 9 Chemical Change Section 9.1 Electrolytes and Solution Conductivity Goal 1 Electrical Conductivity Distinguish among strong electrolytes, weak electrolytes, and nonelectrolytes. Strong Electrolyte:
More informationChapter 3 Chemical Reactions
Chapter 3 Chemical Reactions Jeffrey Mack California State University, Sacramento Chemical Reactions Reactants: Zn + I 2 Product: ZnI 2 Chemical Reactions Evidence of a chemical reaction: Gas Evolution
More informationExam III Material Chapter 7-CHEMICAL REACTIONS, continued
Exam III Material Chapter 7-CHEMICAL REACTIONS, continued A chemical reaction occurs when there is a change in chemical composition. I. Double Replacement/Double Exchange/Metathesis Reactions In an double
More informationed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13
ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)
More informationCHEMICAL REACTIONS. There are three ways we write chemical equations. 1. Molecular Equations 2. Full Ionic Equations 3. Net Ionic Equations
CHEMICAL REACTIONS Reactants: Zn + I 2 Product: Zn I 2 Unit 2 Chemical Reactions The unit 2 exam will cover material from multiple chapters. You are responsible for the following from your text on exam
More information9/24/09 Chem 111 Experiment #7 Solutions and Reactions Brown, LeMay, and Bursten Chapter
Chem 111 Experiment #7 Solutions and Reactions Brown, LeMay, and Bursten Chapter 4.1-4.4 KEY VOCABULARY: 1. Ionic compound a compound composed of cations (+) and anions (-). Many ionic compounds dissociate
More informationAP Chemistry Unit #4. Types of Chemical Reactions & Solution Stoichiometry
AP Chemistry Unit #4 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to: Predict to some extent whether a substance will be a strong electrolyte,
More informationD O UBLE DISPL Ac EMENT REACTIONS
Experiment 8 Name: D O UBLE DISPL Ac EMENT REACTIONS In this experiment, you will observe double displacement reactions and write the corresponding balanced chemical equation and ionic equations. Double
More informationChemistry 101 Chapter 4 STOICHIOMETRY
STOICHIOMETRY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant is necessary
More informationChapter 5 Chemical Reactions
Chapter 5 Chemical Reactions 5.1 Chemical Equations A chemical equation shows the chemical change taking place. The state of each substance is written in parentheses after the formula: s for solids, l
More informationFunsheet 9.1 [VSEPR] Gu 2015
Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NI 3 CF 4 OCl 2 C 2 F 2 HOF Funsheet 9.1 [VSEPR] Gu 2015
More informationEXAM 3 CHEM 1310 WS09 Key Version #2
EXAM 3 CHEM 1310 WS09 Key Version #2 1. (p. 116) Select the correct name and chemical formula for the precipitate that forms when the following reactants are mixed. CuCl 2 (aq) + Na 2 CO 3 (aq) A. copper(ii)
More informationChemistry 150/151 Review Worksheet
Chemistry 150/151 Review Worksheet This worksheet serves to review concepts and calculations from first semester General Chemistry (CHM 150/151). Brief descriptions of concepts are included here. If you
More informationIons in Solution. Solvent and Solute
Adapted from Peer-led Team Learning Begin at the beginning and go on till you come to the end: then stop." Early ideas of atoms and compounds, developed primarily through the reactions of solids and gases,
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions Chapter 4 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A solution is a homogenous mixture of 2 or more substances. The solute
More information(50 pts.) 26. (24 pts.) 27. (8 pts.) 28. (18 pts.) TOTAL (100 points)
Moorpark College Chemistry 11 Spring 2011 Instructor: Professor Torres Examination #2: Section Two March 12, 2011 Name: (print) Name: (sign) Directions: Make sure your examination contains ELEVEN total
More informationCH 4 AP. Reactions in Aqueous Solutions
CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,
More informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred: Temperature change Different coloured materials
More informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
More informationAP Chemistry Honors Unit Chemistry #4 2 Unit 3. Types of Chemical Reactions & Solution Stoichiometry
HO AP Chemistry Honors Unit Chemistry #4 2 Unit 3 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to:! Predict to some extent whether a substance
More informationChapter 4. Reactions In Aqueous Solution
Chapter 4 Reactions In Aqueous Solution I) General Properties of Aqueous Solutions Homogeneous mixture on a molecular level - prop. same throughout - separable by physical means - variable composition
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Micro World atoms & molecules Macro World grams Atomic mass is the mass of an atom in
More information