Limiting Reactants and % Yield

Slides:

Advertisements

Similar presentations

Stoichiometric Calculations

Advertisements

Chapter 3 Atomic masses Average atomic mass –Ex. What is the avg. atomic mass of a sample that is 69.09% amu and 30.91% amu? –0.6909(62.93amu)

Stoichiometry Ratios The stoichiometric coefficients in a balanced chemical reaction can be used to determine the mole relationships between any combination.

Limiting Reactants and Percent Yield

General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake 6.8 Percent Yield and Limiting Reactants Chapter 6 Chemical Reactions and Quantities.

CHAPTER 11 Stoichiometry 11.3 Limiting Reactants.

Chemical Quantities Chapter 9

Limiting Reactants and Excess

Limiting Reagents and Percent Yield

Section Limiting Reagent and Percent Yield

Limiting Reactant and Percent Yield Limiting Reagent u If you are given one dozen loaves of bread, a gallon of mustard and three pieces of salami, how.

Limiting and Excess Reagents

Stoichiometry Limiting Reactants. Stoichiometry Stoichiometry enables us to compare amounts of two substances in a balanced chemical reaction.

Lecture 109/21/05. Mass reactant Stoichiometric factor Moles reactant Moles product Mass product Stoichiometric Calculations.

P ERCENT Y IELD. OBJECTIVE I can calculate percent yield of a reaction.

11-3 Limiting Reactants Reactions to this point have had one ingredient in excess. When you are given two or both reactant amounts, you have a limiting.

Stoichiometry Chapter 9.

Limiting Reactants and % Yield Limiting Factors zLimiting factors are those factors which control the speed or the outcome of a reaction or a situation.

Using S’mores as a Model To Understand Limiting Reactants.

Limiting Reagents and Percent Yield Limiting Reagent If you are given one dozen loaves of bread, a gallon of mustard and three pieces of salami, how.

Stoichiometry & Limiting Reactants. Stoichiometric Calculations The coefficients in the balanced equation give the ratio of moles of reactants and products.

How do you make a cheese sandwich? 2Bd + Ch  Bd 2 Ch LiNkEd LiNkeD.

Limiting Reagents Stochiometry Chapter 9 Chemical Reactions.

Review Mg + 2 HCl  MgCl 2 + H 2 How many Liters of H 2 would be produced with 56 g Mg?

Jeopardy $100 Stoich Vocab Stoich Calculations Stoich True/False Percent Yield Limiting Reactants $200 $300 $400 $500 $400 $300 $200 $100 $500 $400 $300.

Ch. 9-3 Limiting Reactants & Percent Yield. POINT > Define limiting reactant POINT > Identify which reactant is limiting in a reaction POINT > Define.

Chemistry Chapter 9 - Stoichiometry South Lake High School Ms. Sanders.

Stoichiometry – Ch What would be produced if two pieces of bread and a slice of salami reacted together? + ?

Stoichiometry in the Real World Stoichiometry – Ch. 11.

Stoichiometry From the Greek words “stoicheion” meaning “element”

Chapter 9 STOICHIOMETRY

Unit 8: Stoichiometry: Part 1

Limiting Reactants.

Limiting Reactants.

Limiting and Excess Reactants

Limiting Reactants and % Yield

Limiting reactants and percent yield

HONORS CHEMISTRY Feb 27, 2012.

Limiting Reagents and Percent Yield

Stoichiometry Vocab Theoretical Yield: the calculated amount of product yielded by a reaction (found through stoichiometry) Actual Yield: the actual amount.

Chapter 9 “Stoichiometry”

Chapter 9 “Stoichiometry”

Mathematics of Chemical Equations

Introduction to Stoichiometry with S’Mores!

Chapter 9 Chemical quantities.

Limiting Reactants.

Ch. 9 Notes -- Stoichiometry

Stoichiometry Notes.

II. Stoichiometry in the Real World (p. 368 – 375)

Limiting Reactants.

Chapter 9 “Stoichiometry”

Limiting Reagents and Percent Yield

Limiting reactants and percent yield

Warm-up 5.11 S’MORES FACTORY

Chemistry – April 20, 2018 P3 Challenge –

Give me S’MORE Stoichiometry!

Stoichiometry & Limiting Reactants

Chemistry – April 23, 2018 P3 Challenge –

Limiting Reagent If you are given one dozen loaves of bread, a gallon of mustard and three pieces of salami, how many salami sandwiches can you make? The.

CHAPTER 12.2 BASIC STOICHIOMETRY

Limiting Reactants.

Limiting Reagents.

Chapter 9 “Stoichiometry”

LIMITING REAGENT (LR) gets completely used up in the reaction

Presentation transcript:

Limiting Reactants and % Yield

Limiting Factors Limiting factors are those factors which control the speed or the outcome of a reaction or a situation Ingredients for making “S’mores”: 2 graham crackers 1 marshmallow 1 Hershey bar How many “S’mores” can you make with 14 graham crackers, 5 marshmallows, and 6 Hershey bars? How many of each ingredient are left over? 5 “S’mores”, 0 marshmallows, 4 graham crackers, 1 Hershey bar

Limiting Reactant Excess The limiting reactant is the reactant which controls the rate of reaction or the amount of product that can be made The reactant that you have more than you need to perform a chemical reaction

Here’s an example You are making ham and cheese sandwiches and you have: 5 pieces of ham 5 pieces of cheese 8 pieces of bread Which of these ingredients do you have more than enough of (excess reactant)? Which of these do you not have enough of (limiting reactant?

Now lets apply this to an equation… C3H8 + O2  CO2 + H2O Balance the equation How many moles of CO2 are produced from 14.8 g of C3H8? How many moles of CO2 are produced from 3.44 g of O2? If you mixed 14.8 g C3H8 with 3.44 g O2 , which would run out first? (In other words, which one is the limiting reagent?). How do you know? Compare using mole ratio

Yield Yield is how much product that you produce Actual yield refers to the amount of product that is actually generated (measured) Theoretical yield refers to the amount of product that you expect to generate (Calculated)

Theoretical vs. Actual Yield You recently bought a new car. The EPA sticker says that you should get 28 mpg in “average driving”. Your actual miles per gallon turns out to be less than 28 mpg. Why?

Theoretical Yield vs. Actual You perform a mass- mass calculation to determine how much chemical should be produced in a reaction. The actual results of the experiment produce less chemical than calculated. Why?

Calculating Percent Yield Calculate the theoretical yield (mass-mass calculation). Determine the actual yield. Calculate the % yield % Yield = Actual yield x 100 Theoretical yield

A Percent Yield Problem C3H8 + O2  CO2 + H2O In an ideal situation, how many grams of CO2 would be produced? (This is the theoretical yield). If this reaction was carried out and 2.0 g of CO2 were produced (This is the actual yield), what is the percent yield of CO2?