Equation Stoichiometry.notebook. November 23, 2015
|
|
- Tyrone Gibbs
- 5 years ago
- Views:
Transcription
1 1
2 The coefficients in a balanced chemical equation represent moles of reactants and moles of products. The mole ratio (or proportion) of reactants and products in a balanced equation must remain constant. This is how they react stoichiometrically, so to speak. A simple analogy would be in baking a cake. Let s say to bake one cake you need the following ingredients: If you we wanted to bake three cakes, How many eggs would we need? What about the sugar? How many teaspoons of vanilla? Get the idea? 2 eggs 1 cup flour 1 teaspoon vanilla all on left = 1 cake ½ cup of sugar ½ cup of milks by yeast: The same idea applies to the mole ratios of reactants and products in a balanced equation. 2
3 Mole Mole Calculations Given the reaction for the fermentation of simple sugar: C 6H 12O 6(aq) 2 C 2H 5OH(l) + 2 CO 2(g) glucose alcohol carbon dioxide mole ratio: or or Problem 1 How many moles of ethanol (the alcohol) can be produced by the complete fermentation of 12 moles of glucose? Problem 2 How many moles of glucose must be fermented to produce 5 moles of carbon dioxide? 3
4 Mole Mass and Mass Mole Calculations If you understand mole mole idea, a mole mass or mass mole simply involves an additional step of converting mole to mass or mass to mole. Write a balanced equation for the complete combustion of acetylene gas, C 2H 2(g): Problem 3 Calculate the mass of carbon dioxide gas that can be produced by the complete combustion of 10.0 moles of acetylene: Problem 4 How many moles of water can be produced if 104. grams of acetylene completely reacts with oxygen gas? 4
5 Problem 5 Calculate the mass of hydrogen produced by the electrolysis of 25.0 moles of water. Problem 6 Determine the mass of glucose produced by a plant using the photosynthesis reaction if it absorbs 2.00 moles of water. 5
6 Mole Volume Molecules Calculations Recall we learned that one mole of any gas at STP (0 o C and1 atmosphere pressure) occupies a volume of 22.4 liters and that one mole contains Avogadro s number of particles. Let s try some stoichiometry problems involving molecules and gas volumes at STP. Problem 7 Calculate the volume of oxygen gas produced from the decomposition of 2.50 moles of sodium chlorate when the gas is measured at STP: Problem 8 Determine the moles of calcium carbonate that must be decomposed to produce 28.0 L of carbon dioxide gas when the gas is measured at STP: 6
7 Problem 9 Calculate the number of oxygen molecules required to react with g of magnesium metal to produce magnesium oxide. Problem 10 Elemental phosphorous (which occurs as a tetratomic molecule, P 4) reacts with chlorine gas to produce phosphorous trichloride gas. Determine the number of phosphorous molecules and the volume of chlorine gas, when measured at STP, needed to produce 79.5 L of phosphorous trichloride. 7
8 Mass Mass Calculations In this type of problem, we are given the mass of one component in the reaction and asked to calculate the mass of another. These types of problems involve the following conversions: mass A mole A mole B mass B (from coefficients in equation) Problem 11 How many grams of ammonia can be made by reacting 25.0 g of nitrogen with sufficient hydrogen? 8
9 Problem 12 Write a balanced equation for the neutralization of solid magnesium hydroxide by hydrochloric acid. If 5.00 g of solid magnesium hydroxide is swallowed, what mass of hydrochloric can be neutralized? (Caution: do not ingest magnesium hydroxide directly take an antacid tablet containing MOM). Problem 13 If 3.20 g of sodium hydroxide is dissolved in water and reacts with sufficient aqueous copper(ii)chloride, calculate the mass of precipitate that will form. 9
10 Limiting Reactant Problems Thus far we have done stoichiometry problems where we always assumed that the given quantities of reactants in a reaction occurred in stoichiometric amounts. This is not always the case. In a limiting reactant problem, one of the reactants runs out first and is termed the limiting reactant (LR). The LR will thus dictates the amount of products formed. The other reactant(s) is therefore in excess (XS). There are different ways to solve limiting reactant problems, but what most students find easiest is just to apply the mass mass idea in solving these problems. Solve for the mass of one component (usually a product) by assuming the first quantity of reactant given is limiting reactant. Do the same for the second quantity of reactant given. Whichever reactant results in the lower amount of product is the limiting reactant! 10
11 reactant results in the lower amount of product is the limiting reactant! Problem 14 Ethanol, C 2H 5OH, reacts with oxygen gas to produce carbon dioxide and water vapor. If 50.0 g of ethanol reacts with 72.0g of oxygen gas, what mass of carbon diox 1. mass ethanol mole ethanol mole carbon dioxide mass carbon dioxide if ethanol is limiting reactant: 2. mass oxygen mole oxygen mole carbon dioxide mass carbon dioxide if oxygen is limiting reactant: 3. Which reactant will run out first? Which will be in excess (XS)? Now let s calculate the mass of excess reactant left over after the LR runs out. One way to do this is to determine the mass of excess reactant that reacts and subt 11
12 Problem 15 If 25.4 grams of hydrogen gas reacts with 64.8 g of nitrogen gas to produce ammonia gas (NH 3), 1. write a BME 2. determine the LR 3. determine the mass of ammonia produced 4. determine the mass of XS reactant left over 12
13 Percent Yield The percent yield of a reaction is the amount of substance (product) you actually obtain in a reaction divided by the theoretical amount you should obtain X 100. The theoretical amount is the stoichiometric amount we have been calculating in our problems thus far. Problem 16 Hydrogen peroxide can be decomposes to water and oxygen gas. Write a balanced equation for this decomposition below: a) Calculate the volume of oxygen gas that would be produced if 175 g of hydrogen peroxide is decomposed at STP: b) If 51.4 L of oxygen gas is actually obtained, determine the percent yield: 13
14 Problem 17 In the decomposition of exactly g of copper(ii)carbonate, 7.50 g of copper(ii)oxide was obtained (along with the oxygen gas). Calculate the percent yield: 14
15 Energy in Calculations In these problems the energy term (in kilojoules) is in the same proportion as the moles of reactants and moles of products. Let s take an example. Problem 18 According to Reference Table I (found on the last page), 3351 kj of energy is released when 2 moles of aluminum oxide is formed from its elements at kpa and 298 K (these are standard conditions). Write the balanced equation (including the energy term), and calculate the amount of energy that will be released when g of aluminum oxide is formed from its elements. Problem 19 According the Reference Table I, determine the amount of heat energy involved when g of solid sodium hydroxide is dissolved in water. Include a balanced equ 15
16 Problem 20 Calculate the amount of heat energy involved in the reaction of 5.00 g of iodine with excess hydrogen gas. Is the heat released or absorbed? Explain. 16
17 17
Stoichiometry CHAPTER 12
CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. * The balanced equation gives the ratios for the reactants and products. 3 eggs
More informationStoichiometry CHAPTER 12
CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. Jan 16 7:57 AM May 24 10:03 AM * The balanced equation gives the ratios for
More informationProportional Relationships
Stoichiometry Video Proportional Relationships 2 1/4 c. flour 1 tsp. baking soda 1 tsp. salt 1 c. butter 3/4 c. sugar 3/4 c. brown sugar 1 tsp vanilla extract 2 eggs 2 c. chocolate chips Makes 5 dozen
More informationStoichiometry World of Chemistry: Chapter 9
Stoichiometry World of Chemistry: Chapter 9 Chocolate Chip Cookies!! 1 cup butter 1/2 cup white sugar 1 cup packed brown sugar 1 teaspoon vanilla extract 2 eggs 2 1/2 cups all-purpose flour 1 teaspoon
More informationCHAPTER 12. Chemists use balanced to calculate how much reactant is needed or product is formed in a reaction. + 3H 2NH. Hon Chem 12.
CHAPTER 12 Stoichiometry is the calculation of quantities using different substances in chemical equations. Based on the Law of Conservation of Mass. Mg(s) + How many moles of H Chemists use balanced to
More informationOutcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass,
Stoichiometry Outcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass, volume, and heat of reaction. Stoichiometry
More informationChemistry Chapter 9. Unit 6 Stoichiometry
Chemistry Chapter 9 Unit 6 Stoichiometry The arithmetic of equations Equations are recipes. They tell chemists what amounts of reactants to mix and what amounts of products to expect. What is Stoichiometry?
More information2.9 The Mole and Chemical Equations:
2.9 The Mole and Chemical Equations: Stoichiometry Whether you are making omelettes in a kitchen or soap in a factory, you need to know the quantities of ingredients required to produce a certain quantity
More informationSTOICHIOMETRY. Engr. Yvonne Ligaya F. Musico 1
STOICHIOMETRY Engr. Yvonne Ligaya F. Musico 1 Stoichiometry The study in chemistry dealing with calculations based on balanced chemical equations. The branch of chemistry dealing with mass relationships
More informationApply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a
Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a catalyst. CO (g) + H 2 (g) CH 3 OH (l) If 75.0 g of CO reacts
More informationUNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY
UNIT 3 IB MATERIAL Name: BONDING, MOLES & STOICHIOMETRY ESSENTIALS: Know, Understand, and Be Able To Apply the mole concept to substances. Determine the number of particles and the amount of substance
More informationThe Mole. Relative Atomic Mass Ar
STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers
More informationSTOICHIOMETRY. Measurements in Chemical Reactions
STOICHIOMETRY Measurements in Chemical Reactions STOICHIOMETRY Stoichiometry is the analysis of the quantities of substances in a chemical reaction. Stoichiometric calculations depend on the MOLE-MOLE
More informationChapter 3 Stoichiometry
Chapter 3 Sep 22 1:45 PM Average atomic mass: The weighted average of all isotopes of a specific element. Takes into consideration abundance of each isotope. (% x M 1 ) + (% x M 2 ) +... Sep 22 1:45 PM
More information1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen?
Stoichiometry Mole-to-Mole 1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen? N 2 + H 2 NH 3 2. If 5.50 moles of calcium carbide (CaC 2 ) reacts with an excess of
More informationA. Correct. You successfully completed the stoichiometry problem. B. Incorrect. There are 2 moles of AgCl produced for each mole of CaCl 2 reacted.
MCAT General Chemistry Problem Drill 18: Stoichiometry Question No. 1 of 10 1. How many grams of AgCl will precipitate out if 0.27 mole is reacted? + 2 AgNO 3 2 AgCl + Ca(NO 3 ) 2 Question #01 (A) 77 g
More informationA. Correct! You successfully completed the stoichiometry problem.
CLEP Chemistry - Problem Drill 09: Stoichiometry No. 1 of 10 Instructions: (1) Read the problem statement and answer choices carefully () Work the problems on paper as 1. How many grams of AgCl will precipitate
More informationName: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry
Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical
More informationSTOICHIOMETRY ANALOGY
STOICHIOMETRY ANALOGY 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
More informationChemical Reactions and Stoichiometry. Ms. Grobsky
Chemical Reactions and Stoichiometry Ms. Grobsky Wrapping Up the Types of Chemical Reactions We just got done investigating the different types of chemical reactions We can now answer the two questions
More informationStoichiometry. Consider the reaction in which the reactants are nitrogen gas and hydrogen gas. They produce the product ammonia gas.
1 1. Interpreting Chemical Equations Stoichiometry Calculations using balanced equations are called stoichiometric calculations. The starting point for any problem involving quantities of chemicals in
More informationUnit 6: React ions & St oichiom et ry, Chapt er s 11 & 12. Nam e: Period: Description Reaction Types Activty
Unit 6: React ions & St oichiom et ry, Chapt er s 11 & 12 Nam e: Period: Unit Goals- As you work through this unit, you should be able to: 1. Write formula equations from word equations using appropriate
More informationHow many molecules are in 0.25 moles of CH 4?
Mass Moles- Particle Particles can be atoms, molecules, ions, etc. In one mole of particles, there are 6.02x10 23 particles These particles are so small and we need so many of them to be on a human scale,
More informationChem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Chem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 11.1 notes 1 MOLE = 6.02 x 10 23 representative particles representative particles
More informationUnit 6: Stoichiometry. How do manufacturers know how to make enough of their desired product?
Unit 6: Stoichiometry How do manufacturers know how to make enough of their desired product? Chocolate Chip Cookies Using the following recipe, complete the questions. Cookie Recipe 1.5 c sugar 1 c. butter
More informationCh. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles representative particles = ATOMS, IONS,
More informationChapter 3: Chemical Reactions and the Earth s Composition
Chapter 3: Chemical Reactions and the Earth s Composition Problems: 3.1-3.3, 3.5, 3.11-3.86, 3.95-3.115, 3.119-3.120, 3.122, 3.125-3.128, 3.132, 3.134, 3.136-3.138-3.141 3.2 The Mole Stoichiometry (STOY-key-OM-e-tree):
More informationStoichiometry Chapter 9 Practice Assessment B
NAME Hour Date Stoichiometry Chapter 9 Practice Assessment B Objective 1: Interpret balanced chemical equations in terms of interacting moles, representative particles, masses, and gas volume at STP. Directions:
More informationChapter 9: Stoichiometry The Arithmetic ti Of Equations
Chapter 9: Stoichiometry The Arithmetic of Equations Chemical Calculations Limiting Reagent and Percent Yield The Arithmetic ti Of Equations -- The Arithmetic of Equations -- Using Everyday Equations Stoichiometry
More informationChapter 1 IB Chemistry Warm Ups Stoichiometry. Mrs. Hilliard
Chapter 1 IB Chemistry Warm Ups Stoichiometry Mrs. Hilliard Vocabulary 1. Atomic theory 2. Kelvin 3. Mole 4. Relative abundance 5. Molar Mass 6. Empirical formula 7. Molecular formula 8. Stoichiometry
More informationAP Chemistry: Chapter 3 Notes Outline
AP Chemistry: Chapter 3 Notes Outline Objectives: Balance chemical equations Use dimensional analysis to solve stoichiometric problems Use dimensional analysis to do limiting reactant problems Use dimensional
More informationUNIT 1 Chemical Reactions Part II Workbook. Name:
UNIT 1 Chemical Reactions Part II Workbook Name: 1 Molar Volume 1. How many moles of a gas will occupy 2.50 L at STP? 2. Calculate the volume that 0.881 mol of gas at STP will occupy. 3. Determine the
More informationChemistry I Chapter 9 Stoichiometry Objective Sheet. Equation 1. Objectives: 1. Define stoichiometry
Chemistry I Chapter 9 Stoichiometry Objective Sheet Equation 1 2 C 2 H 2 (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O (g), at STP C 2 H 2 (acetylene) 26 g/mol O 2 32 g/mol CO 2 44 g/mol H 2 O 18 g/mol Objectives:
More informationStoichiometric Calculations
Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Table of Contents Click on the topic to go to that section Stoichiometry Calculations with Moles Stoichiometry Calculations with Particles
More informationChapter 9. Table of Contents. Stoichiometry. Section 1 Introduction to Stoichiometry. Section 2 Ideal Stoichiometric Calculations
Stoichiometry Table of Contents Section 1 Introduction to Stoichiometry Section 2 Ideal Stoichiometric Calculations Section 3 Limiting Reactants and Percentage Yield Section 1 Introduction to Stoichiometry
More informationIdeal Gas & Gas Stoichiometry
Ideal Gas & Gas Stoichiometry Avogadro s Law V a number of moles (n) V = constant x n Constant temperature Constant pressure V 1 /n 1 = V 2 /n 2 Ammonia burns in oxygen to form nitric oxide (NO) and water
More informationChemical Reactions. Chemical changes are occurring around us all the time
Chemical changes are occurring around us all the time Food cooking Fuel being burned in a car s engine Oxygen being used in the human body The starting materials are called reactants The ending materials
More informationStoichiometric Calculations
Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Slide 4 / 109 Table of Contents Stoichiometry Calculations with Moles Click on the topic to go to that section Stoichiometry Calculations
More informationName Date Class THE ARITHMETIC OF EQUATIONS
12.1 THE ARITHMETIC OF EQUATIONS Section Review Objectives Calculate the amount of reactants required or product formed in a nonchemical process Interpret balanced chemical equations in terms of interacting
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 informationSTOICHIOMETRY CLASSWORK
STOICHIOMETRY CLASSWORK Given the following equation: 2 C4H10 + 13 02 ---> 8 CO2 + 10 H20 Show what the following molar ratios should be. a, C4H10 / 02 b. 02 / CO2 o, 02 / H20 d, C4Hlo / CO2 e. C4Hlo /
More informationUnit 7: Stoichiometry Homework Packet (85 points)
Name: Period: By the end of the Unit 7, you should be able to: Chapter 12 1. Use stoichiometry to determine the amount of substance in a reaction 2. Determine the limiting reactant of a reaction 3. Determine
More informationName Date Class STUDY GUIDE FOR CONTENT MASTERY
Stoichiometry Section 12.1 What is stoichiometry? In your textbook, read about stoichiometry and the balanced equation. For each statement below, write true or false. 1. The study of the quantitative relationships
More informationCHAPTER 12: STOICHIOMETRY
Name: CHAPTER 12: STOICHIOMETRY Period: MOLE TO MOLE RATIO When nitrogen and hydrogen gas are heated under the correct conditions, ammonia gas (NH 3 ) is formed. a. RXN: 1N 2 + 3H 2 2NH 3 b. How many moles
More informationChemical Reactions Chapter 8 PART TWO
NAME Hour Date Chemical Reactions Chapter 8 PART TWO Practice A Assessment 1 Objective 5: Predict the product of a combination reaction by writing a complete balanced equation. Directions: Write a complete
More informationHonors Chemistry Unit 6 Moles and Stoichiometry Notes. Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number?
Honors Chemistry Unit 6 Moles and Stoichiometry Notes Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number? 3. What does it mean? 4. How is a mole like a dozen doughnuts? Formula
More informationName Date Class. Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line.
12 STOICHIOMETRY Chapter Test B A. Matching Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. 1. 2. 3. 4. 5. Column A the substance
More informationCHAPTER 9 CHEMICAL QUANTITIES
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 9 CHEMICAL QUANTITIES Day Plans for the day Assignment(s) for the day 1 Begin Chapter
More informationChem 11 UNIT 3: STOICHIOMETRY Name:
Chem 11 UNIT 3: STOICHIOMETRY Name: Ms. Pirvu Period: Writing & Balancing Equations Chemical reactions can be described by chemical equations. Recall Law of Conservation of Mass mass cannot be nor. This
More information5. The mass of oxygen required to completely convert 4.0 grams of hydrogen to water is 1) 8.0 grams; 2) 2.0 grams; 3) 32 grams; 4) 16 grams.
CHEMISTRY TEST NAME: MASS AND VOLUME DATE: EQUATION RELATIONSHIPS Directions: For each of the following questions, choose the number that best answers the question and place it on your answer sheet. Directions:
More informationName: Unit 9- Stoichiometry Day Page # Description IC/HW
Name: Unit 9- Stoichiometry Day Page # Description IC/HW Due Date Completed ALL 2 Warm-up IC 1 3 Stoichiometry Notes IC 1 4 Mole Map IC X 1 5 Mole to Mole Practice IC 1 6 Mass to Mole Practice IC 1/2 X
More informationMole Conversions Worksheet
Mole Conversions Worksheet There are three mole equalities. They are: 1 mol = 6.02 x 10 particles 1 mol = g-formula-mass (periodic table) 1 mol = 22.4 L for a gas at STP Each equality can be written as
More informationStoichiometry of Gases
CHAPTER 13 Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations. Many reactions have
More informationExample Exercise 10.1 Interpreting Chemical Equation Calculations
Example Exercise 10.1 Interpreting Chemical Equation Calculations Given the chemical equation for the combustion of methane, CH 4, balance the equation and interpret the coefficients in terms of (a) moles
More informationFinal Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY
Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct
More information4.3 Reaction Stoichiometry
198 Chapter 4 Stoichiometry of Chemical Reactions 4.3 Reaction Stoichiometry By the end of this section, you will be able to: Explain the concept of stoichiometry as it pertains to chemical reactions Use
More informationQuantity Relationships in Chemical Reactions
Chapter 10 Relationships in Chemical Reactions Section 10.1 Conversion Factors from a Chemical Equation Goal 1 The coefficients in a chemical equation give us the conversion factors to get from the number
More informationStoichiometry Part 1
Stoichiometry Part 1 Formulae of simple compounds Formulae of simple compounds can be deduced from their ions/valencies but there are some that you should know off by heart. You will learn these and more
More informationChemical Reactions. Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions. (ionic equations and solubility rules)
Chemical Reactions Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions (ionic equations and solubility rules) Writing Equations REACTANTS PRODUCTS gold (III) sulfide is
More information(DO NOT WRITE ON THIS TEST)
Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation
More informationChapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry
Previous Chapter Table of Contents Next Chapter Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry Section 2.1: The Atomic Mass The atomic mass is the mass of 1 atom. Atoms are
More information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More informationStoichiometry Ch. 11. I. Stoichiometric Calculations
Stoichiometry Ch. 11 I. Stoichiometric Calculations Background on things you NEED to know how to do: 1. Name/write correct chemical formula 2. Write chemical equations 3. Balance chemical equations 4.
More informationReactions and Stoichiometry.
Problem Set Reactions and Stoichiometry. Clearly write answers on separate sheets. Show all work and units. 1. Classify the following chemical reactions according to the categories discussed in class.
More informationStoichiometry Dry Lab
Stoichiometry Dry Lab Name: Mole-Mass Conversions The molar mass of a substance is the conversion factor that allows us to convert between the mass of a substance (in grams) and the number of moles of
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 informationUnit 10: Stoichiometry. Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction.
Unit 10: Stoichiometry Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction. Info given by a chemical equation: Chemical changes involve
More informationBasic Concepts of Chemistry Notes for Students [Chapter 7, page 1] D J Weinkauff - Nerinx Hall High School
Basic Concepts of Chemistry Notes for Students [Chapter 7, page 1] Chapter 7 Quantitative Relationships in Chemical Reactions As you have begun to see, chemistry is a quantitative science involving a great
More informationStoichiometry Dry Lab
Stoichiometry Dry Lab Name: Mole-Mass Conversions The molar mass of a substance is the conversion factor that allows us to convert between the mass of a substance (in grams) and the number of moles of
More informationIB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
More informationCHEMISTRY MOLES PACKET PAGE 1. Chemistry Moles Packet
CHEMISTRY MOLES PACKET PAGE 1 Chemistry Moles Packet CHEMISTRY MOLES PACKET PAGE 2 INTRODUCTION TO MOLES We are about to start on a unit of chemical calculations called stoichiometry. Stoichiometry is
More information4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4
Honors Chemistry Practice Final 2017 KEY 1. Acetylene gas, C 2, is used in welding because it generates an extremely hot flame when combusted with oxygen. How many moles of oxygen are required to react
More informationFunsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017
Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Balance the following chemical equations. Remember, it is not necessary to write "1" if the coefficient is one. 1. N 2 + H 2 NH 3 2. KClO 3 KCl +
More informationCHAPTER 14: The Behavior of Gases
Name: CHAPTER 14: The Behavior of Gases Period: RELATIONSHIPS BETWEEN PRESSURE, VOLUME & TEMPERATURE OF A GAS Boyle s Law-Pressure and Volume Volume (ml) Pressure ( ) 60 50 40 30 20 10 Practice problem:
More information11 Stoichiometry. Section 11.1 What is stoichiometry?
11 Stoichiometry Section 11.1 What is stoichiometry? In your textbook, read about stoichiometry and the balanced equation. For each statement below, write true or false. 1.. 3. 4. 5. The study of the quantitative
More informationIGCSE Double Award Extended Coordinated Science
IGCSE Double Award Extended Coordinated Science Chemistry 4.1 - The Mole Concept The Atomic Mass Unit You need to know the atomic mass unit and the relative atomic mass. In Unit C3.3, 1 atomic mass unit
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 informationStoichiometry. Homework EC. cincochem.pbworks.com. Academic Chemistry DATE ASSIGNMENT
Unit 10 Resournces Name Academic Chemistry Stoichiometry Homework On-Time LATE DATE ASSIGNMENT 100 70 10.1 10.2 10.3 10.4 10.5 10.6 EC 16 cincochem.pbworks.com Stoichiometry Live in the now. Garth Algar
More informationCHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS
Lesson 1 1. (a) Deduce the number of protons, neutrons and electrons in the following species: (i) 37 Cl - (ii) 1 H + (iii) 45 Sc 3+ (b) Write symbols for the following species: (i) 8 protons, 8 neutrons,
More informationAP Chemistry Summer Assignment
AP Chemistry Summer Assignment Due Date: Thursday, September 1 st, 2011 Directions: Show all of your work for full credit. Include units and labels. Record answers to the correct number of significant
More informationLimiting Reactants. and Percentage Yield. Section 3
GO ONLINE Section 3 8E Main Ideas One reactant limits the product of a reaction. Comparing the actual and theoretical yields helps chemists determine the reaction s efficiency. 8E perform stoichiometric
More informationChemistry 2202 Stoichiometry Unit Retest Review Guide
Chemistry 2202 Stoichiometry Unit Retest Review Guide Chapter 2: The Mole Pgs. 42 77 You should be able to: 1. Define the term molar mass and calculate the molar mass of any given element or compound.
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 10 Chemical Equation Calculations by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 10 1 What
More informationChemistry PreAP. Homework Packet. S t o I c h I o m e t r y. Name:
Chemistry PreAP Homework Packet S t o I c h I o m e t r y Name: 1 lj STOICHIOMETRY CLASSWORK Given the following equation: 2 C4H10 + 13 02 o-ÿ> 8 CO2 + 10 H20 Show what the following molar ratios should
More informationCounting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles
Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole
More informationTOPIC 4: THE MOLE CONCEPTS
TOPIC 4: THE MOLE CONCEPTS INTRODUCTION The mass is gram (g) of 1 mole of substances is called its.. 1 mole of substances has.. particles of a substances The mass of 1 mole of substances is always equal
More informationSSLC CHEMISTRY UNIT 2 MOLE CONCEPT - WORK SHEETS WORK SHEET 1
1 SSLC CHEMISTRY UNIT 2 MOLE CONCEPT - WORK SHEETS WORK SHEET 1 1 GAM atoms Mass in grams equal to its Atomic mass Element and GAM Number of Atoms Mass in grams 1 GAM Hydrogen atoms 1 g 1 GAM Helium atoms
More informationTopic 1 Review. Ms. Kiely Coral Gables Senior High IB Chemistry SL
Topic 1 Review Ms. Kiely Coral Gables Senior High IB Chemistry SL Bell-Ringer A 4 g sample of sodium hydroxide, NaOH, is dissolved in water and made up to 500 cm³ of aqueous solution. What is the concentration
More information17.2 Thermochemical Equations
17.2. Thermochemical Equations www.ck12.org 17.2 Thermochemical Equations Lesson Objectives Define enthalpy, and know the conditions under which the enthalpy change in a reaction is equal to the heat absorbed
More informationCHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS
Lesson 1 1. (a) Deduce the number of protons, neutrons and electrons in the following species: (i) 37 Cl - (ii) 1 H + (iii) 45 Sc 3+ (b) Write symbols for the following species: (i) 8 protons, 8 neutrons,
More informationUNIT 3 Quantities in Chemical Reactions THE MOLE!
UNIT 3 Quantities in Chemical Reactions THE MOLE! In chemistry as in other aspects of life it is sometimes more convenient to count in groups of items rather than count items individually. Quantity Amount
More informationName. Academic Chemistry Stoichiometry Notes. Unit #10 Test Date: cincochem.pbworks.com
Name Academic Chemistry Stoichiometry Notes Unit #10 Test Date: cincochem.pbworks.com Resources Unit 10 Common Polyatomic Ions List 20 Name Common Polyatomic Ion Ions Name Ion acetate C 2 H 3 O 2 or CH3
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 informationMoles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitri
Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitride Magnesium phosphate Mole Conversions One-step How
More informationChapter 4: Chemical and Solution Stoichiometry
Chapter 4: Chemical and Solution Stoichiometry (Sections 4.1-4.4) 1 Reaction Stoichiometry The coefficients in a balanced chemical equation specify the relative amounts in moles of each of the substances
More informationUNIT 3 Chemical Quantities Chapter 5 Counting Atoms and Molecules The Mole
UNIT 3 Chemical Quantities Chapter 5 Counting Atoms and Molecules The Mole How does the mass of a substance relate to the number of atoms in the substance? Recall: Atomic mass units. Atomic mass units
More informationA-LEVEL TRANSITION COURSE SUMMER 2018 PART 2: USING CHEMICAL EQUATIONS
A-LEVEL TRANSITION COURSE SUMMER 2018 PART 2: USING CHEMICAL EQUATIONS MASS AQUEOUS VOLUME ` MOLAR MASS GASEOUS VOLUME MOLES CONCENTRATION REVISION FROM LESSON 1 How many moles? 1) Jahin weighs a sample
More informationName: Class: Date: ID: A. (g), what is the ratio of moles of oxygen used to moles of CO 2 produced? a. 1:1 b. 2:1 c. 1:2 d. 2:2
Name: Class: _ Date: _ Chpt 12 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is conserved in the reaction shown below? H 2 + Cl 2 2HCl a.
More information**continued on next page**
Chapter 9 Stoichiometry Section 9.1 Introduction to Stoichiometry Standard.e.: Students know how to calculate the masses of reactant and products in a chemical reaction from the mass of one of the reactants
More informationChapter 3. Stoichiometry
Chapter 3 Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry The study of quantities of materials consumed and produced in chemical reactions. Since atoms are so small, we must use the average
More information