Mole Conversions Worksheet

Size: px
Start display at page:

Download "Mole Conversions Worksheet"

Transcription

1 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 a set of two conversion factors. They are: 1 mole 6.02x10 particles 6.02x10 particles 1 mole g 1 mole formula mass g formula mass 1 mole 1 mole 22.4 L 22.4 L 1 mole Mole-Particle Conversions 1. How many moles of magnesium is 3.01 x atoms of magnesium? 3.01 x mole atoms 6.02x10 atoms = 5 x 10-2 moles 2. How many molecules are there in 4.00 moles of glucose, C 6 H 12 O 6? 3. How many moles are 1.20 x atoms of phosphorous? 4. How many atoms are in moles of zinc? 5. How many molecules are in moles of N 2 O 5? Mole-Mass Conversions 1. How many moles in 28 grams of CO 2? Gram-formula-mass of CO 2 1 C = 1 x g = g 2 O = 2 x g = g g/mol 1 mole 28 g CO 2 = 0.64 moles CO g

2 2. What is the mass of 5 moles of Fe 2 O 3? Gram-formula-mass Fe 2 O 3 2 Fe = 2 x 55.6 g = g 3 O = 3 x 16.0 g = 48.0 g g/mol g 5 moles Fe 2 O 3 1 mole = 800 grams Fe2O3 3. Find the number of moles of argon in 452 g of argon. 4. Find the grams in 1.26 x 10-4 mol of HC 2 H 3 O Find the mass in 2.6 mol of lithium bromide. Mole-Volume Conversions 1. Determine the volume, in liters, occupied by moles of a gas at STP L mol 1 mole = 0.67 L 2. How many moles of argon atoms are present in 11.2 L of argon gas at STP? 1 mole 11.2 L 22.4 L = moles 3. What is the volume of 0.05 mol of neon gas at STP? 4. What is the volume of 1.2 moles of water vapor at STP?

3 Mixed Mole Conversions Given unit Moles Desired unit 1. How many oxygen molecules are in 3.36 L of oxygen gas at STP? 1 mole 3.36 L 6.02x10 molecules 22.4 L 1 mole = 9.03 x molecules 2. Find the mass in grams of 2.00 x 10 molecules of F g 3. Determine the volume in liters occupied by 14 g of nitrogen gas at STP. 4. Find the mass, in grams, of 1.00 x 10 molecules of N How many particles are there in 1.43 g of a molecular compound with a gram molecular mass of 3 g? 6. Aspartame is an artificial sweetener that is 160 times sweeter than sucrose (table sugar) when dissolved in water. It is marketed by G.D. Searle as Nutra Sweet. The molecular formula of aspartame is C 14 H 18 N 2 O 5. a) Calculate the gram-formula-mass of aspartame. b) How many moles of molecules are in 10 g of aspartame? c) What is the mass in grams of 1.56 moles of aspartame? d) How many molecules are in 5 mg of aspartame? e) How many atoms of nitrogen are in 1.2 grams of aspartame?

4 AP Chemistry Chemical Equations and Stoichiometry Supplemental Worksheet Name: Date: Period: 1. Oil paintings in which white lead has been used can be blackened by reaction with H 2 S from air pollution or from the glaze over the painting itself. The blackening comes from the formation of lead sulfide, which may be cleaned off by washing with hydrogen peroxide, H 2 O 2. The reaction for the cleaning process is PbS (black solid) + 4 H 2 O 2(aq) PbSO 4(s) + 4 H 2 O (l) a. How many grams of H 2 O 2 must be used to clean off 0.24 g of PbS? b. If g of H 2 O form in the reaction, how many grams of PbSO 4 must also have been formed? 2. Methyl alcohol, CH 3 OH, is a clean-burning, easily handled fuel. It can be made by the direct reaction of CO and H 2 (obtained from coal and water). CO (g) + 2 H 2(g) CH 3 OH (l) Assume you start with 12.0g of H 2 and 74.5g of CO; a. Which of the reactants is in excess? b. Which is the limiting reagent? c. What mass (in grams) of the excess reagent is left after the reaction is complete? d. How many grams of methyl alcohol can be obtained theoretically? 3. Zinc and chlorine react directly to give zinc chloride. Zn (s) + Cl 2(g) ZnCl 2(s) If you begin with 1.00 mole of zinc and excess Cl 2, what is the theoretical yield of ZnCl 2 in grams? If you isolate 115g of ZnCl 2, what is the percent yield of the metal chloride? 4. Butane, which contains only C and H, is a commonly used fuel in camping stoves. To determine the formula of butane, assume you burn 0.580g of the gas and obtain 1.760g of CO 2 and 0.900g of H 2 O. What is the empirical formula of butane? 5. Metal carbonates give the appropriate metal oxide and CO 2 when heated. For example, CaCO 3(s) CaO (s) + CO 2(g) Limestone is mostly calcium carbonate, CaCO 3, but other minerals are usually present as well. Assume a 1.605g sample of limestone is heated and decomposed completely to CaO, g of CO 2, and an inert residue. What is the weight percentage of CaCO 3 in the limestone sample?

5 6. Complete combustion of 0.255g of an alcohol produces grams of CO 2 and grams of H 2 O. Calculate its a. Mass percent composition b. Empirical formula 7. Balance the following equations: PCl 5 + H 2 O H 3 PO 4 + HCl CaO + P 4 O 10 Ca 3 (PO 4 ) 2 Ba(NO 3 ) 2 + Al 2 (SO 4 ) 3 BaSO 4 + Al(NO 3 ) 3 NaHCO 3 + H 2 SO 4 Na 2 SO 4 + H 2 O + CO 2 C 4 H 10 + O 2 CO 2 + H 2 O 8. Write a plausible chemical equation for the combustion of liquid triethylene glycol in an abundant supply of oxygen gas. Triethylene glycol is 47.99% C, 9.40% H, and 42.62% O by mass and has a molecular mass of 150.2u. 9. One way to change the iron mineral, Fe 2 O 3, into metallic iron is to heat it with hydrogen. Fe 2 O 3 + 3H 2 2Fe + 3H 2 O a. How many moles of iron are made from 20mol of Fe 2 O 3? b. How many moles of H 2 are needed to make 24mol of Fe? c. If 90mol of H 2 O forms, how many grams of Fe 2 O 3 were used up? 10. Phosphorus pentachloride reacts with water to give phosphoric acid and hydrochloric acid. In one experiment, 0.360mol of phosphorus pentachloride was slowly added to 2.88mol of water. a. Which reactant, if either, was the limiting reactant? b. Calculate the theoretical yields (in moles) of phosphoric acid and hydrochloric acid. 11. Aluminum sulfate can be made by the following reaction 2AlCl 3(aq) + 3H 2 SO 4(aq) Al 2 (SO 4 ) 3(aq) + 6HCl (aq) Aluminum sulfate is quite soluble in water, so to isolate it the solution has to be evaporated to dryness. This drives off the volatile HCl, but the residual solid has to be heated to a little over 200 o C to drive off all of the water. In one experiment, 25.00g of AlCl 3 was used. a. How many grams of H 2 SO 4 are needed? b. After the procedure, 28.36g of pure aluminum sulfate was isolated. Calculate the percent yield of the reaction.

UNIT 1 Chemical Reactions Part II Workbook. Name:

UNIT 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 information

Name: 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: 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

Slide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date»

Slide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date» Slide 1 / 90 Stoichiometry HW Grade:«grade» Subject: Date:«date» Slide 2 / 90 1 The calculation of quantities in chemical equations is called. A B C D E accuracy and precision dimensional analysis percent

More information

Stoichiometry. The quantitative study of reactants and products in a chemical reaction. Burlingame High School Chemistry

Stoichiometry. The quantitative study of reactants and products in a chemical reaction. Burlingame High School Chemistry Stoichiometry The quantitative study of reactants and products in a chemical reaction 1 Stoichiometry Whether the units given for reactants or products are moles, grams, liters (for gases), or some other

More information

e) How many atoms of nitrogen are in 1.2 g aspartame? #11 HC 4 of 4

e) How many atoms of nitrogen are in 1.2 g aspartame? #11 HC 4 of 4 Ch. 3 Honors Chem HW #11 HC 1 of 4 A2) An element is a mixture of two isotopes. One isotope of the element has an atomic mass of 34.96885 amu and has a relative abundance of 75.53%. The other isotope has

More information

Balancing Equations Notes

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

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

Name: Unit 9- Stoichiometry Day Page # Description IC/HW

Name: 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 information

Final 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 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 information

Stoichiometry CHAPTER 12

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 information

Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017

Funsheet 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 information

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

2. 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 information

5. 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.

5. 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 information

actual yield (p. 372) excess reagent (p. 369) mole-mole relationship for ag bw: x mol G b mol W a mol G xb a mol W Organizing Information

actual yield (p. 372) excess reagent (p. 369) mole-mole relationship for ag bw: x mol G b mol W a mol G xb a mol W Organizing Information 12 Study Guide 12 Study Guide Study Tip Prioritize Schedule your time realistically. Stick to your deadlines. If your class subscribes to the Interactive Textbook with ChemASAP, your students can go online

More information

Stoichiometry CHAPTER 12

Stoichiometry 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 information

1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen?

1. 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 information

Balancing Equations Notes

Balancing Equations Notes . Unit 6 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

Name 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.

Name 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 information

4. Magnesium has three natural isotopes with the following masses and natural abundances:

4. Magnesium has three natural isotopes with the following masses and natural abundances: Exercise #1. Determination of Weighted Average Mass 1. The average mass of pennies minted after 1982 is 2.50 g and the average mass of pennies minted before 1982 is 3.00 g. Suppose that a bag of pennies

More information

General Chemistry 1 CHM201 Unit 2 Practice Test

General 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 information

Balancing Equations Notes

Balancing Equations Notes . Unit 7 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting

More information

CHAPTER 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. 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 information

Counting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles

Counting 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 information

Honors 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? 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 information

1) Write the reaction for Calcium and nitrogen reacting. 3) What element on the periodic table is the largest? 3)Name these. a) H2S (aq) b) HNO 3 (aq)

1) Write the reaction for Calcium and nitrogen reacting. 3) What element on the periodic table is the largest? 3)Name these. a) H2S (aq) b) HNO 3 (aq) 1) Write the reaction for Calcium and nitrogen reacting 3) What element on the periodic table is the largest? 3)Name these a) H2S (aq) b) HNO 3 (aq) Stoichiometry: mathematical relationships in formulas

More information

CHAPTER 9 CHEMICAL QUANTITIES

CHAPTER 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 information

AP Chemistry Summer Assignment

AP 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 information

The Mole. Relative Atomic Mass Ar

The 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 information

UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY

UNIT 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 information

Advanced Placement Chemistry ~ Summer Assignment Part 2. Name

Advanced Placement Chemistry ~ Summer Assignment Part 2. Name Advanced Placement Chemistry ~ Summer Assignment Part 2 Name Topic 1: Measurements and Dimensional Analysis Appropriately read and report a measurement correctly with one uncertain digit. State the number

More information

During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:

During 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 information

Study Guide: Stoichiometry

Study Guide: Stoichiometry Name: Study Guide: Stoichiometry Period: **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE

More information

Chapter 1 IB Chemistry Warm Ups Stoichiometry. Mrs. Hilliard

Chapter 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 information

Chapter 3 The Mole and Stoichiometry

Chapter 3 The Mole and Stoichiometry Chapter 3 The Mole and Stoichiometry Chemistry, 7 th Edition International Student Version Brady/Jespersen/Hyslop Brady/Jespersen/Hyslop Chemistry7E, Copyright 015 John Wiley & Sons, Inc. All Rights Reserved

More information

2. In which of these compounds are there twice as many oxygen atoms as hydrogen atoms? a. H 3 PO 4 c. HClO 3 b. H 2 SO 4 d. H 2 O

2. In which of these compounds are there twice as many oxygen atoms as hydrogen atoms? a. H 3 PO 4 c. HClO 3 b. H 2 SO 4 d. H 2 O Test Review Unit 3_3: Law of conservation of mass Identify the letter of the choice that best completes the statement or answers the question. At the end of the file you can find chemical equations to

More information

Chem 1A Dr. White Fall Handout 4

Chem 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 information

AP Chapter 3 Study Questions

AP Chapter 3 Study Questions Class: Date: AP Chapter 3 Study Questions True/False Indicate whether the statement is true or false. 1. The mass of a single atom of an element (in amu) is numerically EQUAL to the mass in grams of 1

More information

AP Chemistry: Chapter 3 Notes Outline

AP 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 information

Unit 9 Stoichiometry Notes

Unit 9 Stoichiometry Notes Unit 9 Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations to

More information

Sophomore AP Chem Practice Problems

Sophomore AP Chem Practice Problems Due on 8/17/18 Sophomore AP Chem Practice Problems Scientific notation and significant figures Determine the number of Significant Figures in the following numbers: 00034 2431. 8900 0.0094 Convert the

More information

ACP Chemistry (821) - Mid-Year Review

ACP Chemistry (821) - Mid-Year Review ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference

More information

AP Chemistry Summer Assignment

AP Chemistry Summer Assignment Name AP Chemistry Summer Assignment Welcome to AP chemistry! This summer assignment is intended to help you review the basic topics you learned in pre-ap chemistry that are crucial for your success in

More information

Unit 1 Atomic Structure

Unit 1 Atomic Structure Unit 1 Atomic Structure Unit 1 Text Questions 1.1 Atoms/Ions/Isotopes Problems Ch 5 Prob: 9,23,24,38 1.2 Average Atomic Mass Problems Ch 5 Prob: 15,17 1.3 Atomic Theory Development Problems Ch 5 Prob:

More information

Unit 4: Reactions and Stoichiometry

Unit 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 information

WORKSHEET Mole Fraction

WORKSHEET Mole Fraction NAME: DATE: PERIOD: WORKSHEET Mole Fraction 1. What is the mole fraction of sodium chloride in a solution containing 0.23 moles of NaCl and 5.5 moles of water? 2. What is the mole fraction of oxygen in

More information

Stoichiometric Calculations

Stoichiometric 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 information

Stoichiometric Calculations

Stoichiometric 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 information

THE MOLE - PART 2. Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

THE MOLE - PART 2. Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. THE MOLE - PART 2 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which one of the following statements is a quantitative observation? a.

More information

Unit Two Worksheet WS DC U2

Unit Two Worksheet WS DC U2 Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed

More information

Chemical Reactions Unit

Chemical Reactions Unit Name: Hour: Teacher: ROZEMA / Chemistry Chemical Reactions Unit 1 P a g e 2 P a g e 3 P a g e 4 P a g e 5 P a g e 6 P a g e Chemistry Balancing Equations Balance the following equations by inserting the

More information

How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg?

How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg? 1 A 2 B 3 C The atomic number of Na is 11. How many electrons are there in a sodium ion, Na +? How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? What is the mass in grams

More information

Chapter 9: Stoichiometry The Arithmetic ti Of Equations

Chapter 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 information

Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas

Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas In Chemistry, a Mole is: the unit that measures the amount of a substance - equals 6.022 x 10 23 particles of

More information

Unit 1 SOME BASIC CONCEPTS OF CHEMISTRY I. Multiple Choice Questions (Type-I) 1. Two students performed the same experiment separately and each one of them recorded two readings of mass which are given

More information

Unit 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: 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 information

Stoichiometry ( ) ( )

Stoichiometry ( ) ( ) Stoichiometry Outline 1. Molar Calculations 2. Limiting Reactants 3. Empirical and Molecular Formula Calculations Review 1. Molar Calculations ( ) ( ) ( ) 6.02 x 10 23 particles (atoms or molecules) /

More information

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia Unit 9: The Mole- Funsheets Part A: Molar Mass Write the formula AND determine the molar mass for each of the following. Be sure to include units and round you answer to 2 decimal places. 1) calcium carbonate

More information

Chem. 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. 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 information

Name Date Class. representative particle molar mass representative particles

Name Date Class. representative particle molar mass representative particles 10.1 THE MOLE: A MEASUREMENT OF MATTER Section Review Objectives Relate Avogadro s number to a mole of a substance Calculate the mass of a mole of any substance Describe methods of measuring the amount

More information

CH 221 Chapter Four Part I Concept Guide

CH 221 Chapter Four Part I Concept Guide 1. Balancing Chemical Equations CH 221 Chapter Four Part I Concept Guide Description When chlorine gas, Cl 2, is added to solid phosphorus, P 4, a reaction occurs to produce liquid phosphorus trichloride,

More information

CH 221 Chapter Four Part II Concept Guide

CH 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 information

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO AP Chemistry Summer Review Packet 2018 Section 1: Names and Formulas of ionic compounds. Name: Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic

More information

IB 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.

IB 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 information

Ch. 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. 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 information

Chapter 4. Aqueous Reactions and Solution Stoichiometry

Chapter 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 information

TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry.

TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry. TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry. Stoichiometric calculations. By combining a knowledge of balancing equations with the concept of the mole, it is possible to easily calculate the masses

More information

Name Date Class THE ARITHMETIC OF EQUATIONS

Name 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 information

MIDTERM REVIEW. UNIT 1: Mass/Measurement

MIDTERM REVIEW. UNIT 1: Mass/Measurement MIDTERM REVIEW UNIT 1: Mass/Measurement Practice Problems 1. Circle the word/phrase that best fits the statement: A. [ PHYSICAL OR CHEMICAL] changes are changes in which the identity of the substance does

More information

Chemistry 2202 Stoichiometry Unit Retest Review Guide

Chemistry 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 information

4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4

4 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 information

Chemistry 142A, Autumn 2011 Worksheet #3 Answer Key Ch. 3, start of Ch. 4

Chemistry 142A, Autumn 2011 Worksheet #3 Answer Key Ch. 3, start of Ch. 4 Chemistry 142A, Autumn 2011 Worksheet #3 Answer Key Ch. 3, start of Ch. 4 1) There are several important compounds that contain only nitrogen and oxygen. Calculate the mass percent of nitrogen in each

More information

Section EXAM III Total Points = 150. November 15, Each student is responsible for following directions. Read this page carefully.

Section EXAM III Total Points = 150. November 15, Each student is responsible for following directions. Read this page carefully. Name Chemistry 11100 Test 66 Section EXAM III Total Points = 150 TA Thursday, 8:00 PM November 15, 2012 Directions: 1. Each student is responsible for following directions. Read this page carefully. 2.

More information

Calculations with Chemical Formulas and Equations

Calculations with Chemical Formulas and Equations Calculations with Chemical Formulas and Equations Mass and Moles of a Substance Chemistry requires a method for determining the numbers of molecules in a given mass of a substance. This allows the chemist

More information

Chapter 3. Stoichiometry

Chapter 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

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,

More information

Quantitative Chemistry. AQA Chemistry topic 3

Quantitative Chemistry. AQA Chemistry topic 3 Quantitative Chemistry AQA Chemistry topic 3 3.1 Conservation of Mass and Balanced Equations Chemical Reactions A chemical reaction is when atoms are basically rearranged into something different. For

More information

Unit 6: Mole Assignment Packet Period:

Unit 6: Mole Assignment Packet Period: Unit 6: Mole Assignment Packet Name: Period: A1: Mole Conversions 1. Identify the representative particle in each of the following: (atom, molecule, formula unit) a. CuSO 4 b. H 2 O c. NaCl d. Zn e. Cu

More information

Chapter 5 Chemical Calculations

Chapter 5 Chemical Calculations Calculating moles Moles and elements Moles and compounds Moles and gases Moles and solutions Calculating formulae Finding the formula Chapter 5 Chemical Calculations Moles and chemical equations Checklist

More information

Stoichiometry. The study of quantities of substances in chemical reactions

Stoichiometry. The study of quantities of substances in chemical reactions Stoichiometry The study of quantities of substances in chemical reactions Interpreting Chemical Equations N 2 + 3 H 2 2 NH 3 Particles: 1 molecule of Nitrogen reacts with 3 molecules of Hydrogen to produce

More information

AP Chemistry Chapter 3. Stoichiometry

AP Chemistry Chapter 3. Stoichiometry AP Chemistry Chapter 3 Stoichiometry Stoichiometry Is the study of the quantities of substances consumed and produced in chemical reactions Derived from the Greek words stoicheion meaning element and metron

More information

Stoichiometry. Homework EC. cincochem.pbworks.com. Academic Chemistry DATE ASSIGNMENT

Stoichiometry. 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 information

Slide 1 / 90. Slide 2 / 90. Slide 3 / 90 A B. percent yield stoichiometry A B. atoms and mass

Slide 1 / 90. Slide 2 / 90. Slide 3 / 90 A B. percent yield stoichiometry A B. atoms and mass Stoichiometry HW Slide 1 / 90 Grade:«grade» Subject: ate:«date» 1 The calculation of quantities in chemical equations is called. Slide 2 / 90 accuracy and precision dimensional analysis percent composition

More information

Chemical Reactions. Chemical changes are occurring around us all the time

Chemical 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 information

AP Chemistry Semester 1 Practice Problems

AP Chemistry Semester 1 Practice Problems AP Chemistry Semester 1 Practice Problems 1. Adipic Acid contains 49.32% C, 43.84% O, and 6.85% H by mass. What is the empirical formula? a) C 3 H 5 O 2 b) C 3 H 3 O 4 c) C 2 HO 3 d) C 2 H 5 O 4 e) C 3

More information

Unit 5. Chemical Composition

Unit 5. Chemical Composition Unit 5 Chemical Composition Counting by Mass Individually mass a few Calculate the average mass of one Can count large numbers of by mass Atomic Mass Unit (amu) 1 amu = 1.66 x 10-24 g Subatomic particles

More information

AP WORKSHEET 4s: Calculations Summary

AP WORKSHEET 4s: Calculations Summary AP WORKSHEET 4s: Calculations Summary TYPE 1: Those involving Avogadro s number (the mole concept). Question 1 A sample of Ge is found to contain 9.7 x 10 23 atoms of Ge. How many moles of Ge atoms are

More information

Chemical Equation Calculations

Chemical Equation Calculations Mole Relationships Chemical Equation Calculations 1. How many moles of chlorine gas react with 1 mol of hydrogen gas according to the balanced chemical equation? (a) 1 mol (b) 2 mol (c) 3 mol (d) 4 mol

More information

TOPIC 4: THE MOLE CONCEPTS

TOPIC 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 information

The ions/polyatomic ions, solubility rules, and activity series will need to be memorized.

The ions/polyatomic ions, solubility rules, and activity series will need to be memorized. AP Chemistry Summer Assignment 2012 The summer assignment is designed to help you practice: - writing chemical formulas, names, and chemical equations - reaction types - predicting reaction products -

More information

UNIT 9 - STOICHIOMETRY

UNIT 9 - STOICHIOMETRY General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount

More information

Gravimetric Analysis (Analysis by Mass)

Gravimetric Analysis (Analysis by Mass) Week 2 Measuring water content Gravimetric Analysis (Analysis by Mass Water is a component in many consumer products It may occur naturally or may be added in manufacturing Water content can reveal the

More information

9.) A chloride of rhenium contains 63.6% rhenium. What is the formula of this compound? (ReCl 3 )

9.) A chloride of rhenium contains 63.6% rhenium. What is the formula of this compound? (ReCl 3 ) Homework Stoichiometry 1.) An oxide of iron has the formula Fe 3 O 4. What mass percent of iron does it contain? (72.360%) 2.) Hydrocortisone valerate is an ingredient in hydrocortisone cream, prescribed

More information

Questions Q1. Which of the following contains the greatest number of hydrogen atoms? 2 moles of water, H 2 O. B 1.5 moles of ammonia, NH 3

Questions Q1. Which of the following contains the greatest number of hydrogen atoms? 2 moles of water, H 2 O. B 1.5 moles of ammonia, NH 3 Questions Q1. Which of the following contains the greatest number of hydrogen atoms? 2 moles of water, H 2 O B 1.5 moles of ammonia, NH 3 C 1 mole of hydrogen gas, H 2 D 0.5 moles of methane, CH 4 Q2.

More information

Types of Reactions. There are five types of chemical reactions we observed in the lab:

Types of Reactions. There are five types of chemical reactions we observed in the lab: Chemical Reactions Acids and Bases Acids: Form hydrogen ions (H + ) when dissolved in water. HCl (aq) H + (aq) + Cl - (aq) Examples: HCl (hydrochloric acid), HNO 3 (nitric acid), H 2 SO 4 (sulfuric acid),

More information

1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?

1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3? 1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K

More information

1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D %

1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D % 1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A. 9.372 % C. 28.12 % B. 21.38 % D. 42.73 % 2. How many grams of phosphorus are in 35.70 g of P 2 O 5? A. 6.359 g C. 15.58 g B. 23.37 g D. 31.16

More information

(DO NOT WRITE ON THIS TEST)

(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 information

Stoichiometry. Percent composition Part / whole x 100 = %

Stoichiometry. Percent composition Part / whole x 100 = % Stoichiometry Conversion factors 1 mole = 6.02 x 10 23 atoms (element) 1 mole = 6.02 x 10 23 molecules (covalent compounds) 1 mole = 6.02 x 10 23 formula units (ionic compounds) 1 mole (any gas @ STP)

More information

Get out a sheet of paper to take some notes on.

Get out a sheet of paper to take some notes on. Bellwork: Get out your old textbook and your ID. Get out a sheet of paper to take some notes on. Solve the following problem. Methyl alcohol, CH 3 OH, is a clean-burning, easily handled fuel. It can be

More information

AP Chemistry Unit 3- Homework Problems Gas Laws and Stoichiometry

AP Chemistry Unit 3- Homework Problems Gas Laws and Stoichiometry AP Chemistry Unit 3- Homework Problems Gas Laws and Stoichiometry STP 1. What is standard pressure for each of the following: atm, mm Hg, Torr, kpa, PSI 2. Convert each of the following: a. 700 mm Hg to

More information