Stoichiometry and the Math of Equations Part 4: Percent Yield 1.

Slides:

Advertisements

Similar presentations

II. Stoichiometry in the Real World (p ) Stoichiometry – Ch. 9.

Advertisements

Chapter 5 Chemical Reactions

Chapter 9: Stoichiometry

Chapter 9: Chemical quantities Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor.

Limiting Reactant. Which will run out first? In the real world, one reactant will be consumed before other(s) In the real world, one reactant will be.

Chemistry 11 Chapter 6 STOICHIOMETRY OF EXCESS QUANTITIES.

Chemical Quantities Chapter 9

Stoichiometry: Calculations with Chemical Equations.

Limiting Reagent What happens in a chemical reaction, if there is an insufficient amount of one reactant?

Ppt 12 Plan (PS5, material) 1.Limiting Reactant Situations 2.% Yield 3.Molarity (done in lab—Exp. 24; worksheet in next Ppt) 1Ppt 12.

Stoichiometry, Limiting Reactants and Percent Yield

Chemical Reactions Unit

Stoichiometry Introduction.

Limiting Reagent and Percent Yield

Chapter 9 Chemical Quantities. 9 | 2 Information Given by the Chemical Equation Balanced equations show the relationship between the relative numbers.

Percent Yield and Limiting Reactants

Stoichiometry Percent Yield. Important Terms  Yield: the amount of product  Theoretical yield: the maximum amount of product expected, based on stoichiometric.

Limiting/Excess Reactants and Percent Yield

Limiting Reactants and Percent Yields

Limiting Reactants and Excess

Section 9.1 Using Chemical Equations 1.To understand the information given in a balanced equation 2.To use a balanced equation to determine relationships.

Limiting Reagents and Percent Yield

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

Chemistry 11 Stoichiometry Reality II: Percent Yield.

Ch. 9: Calculations from Chemical Equations

Percent Yield. Theoretical Yield The theoretical yield is the amount of product that can be made –In other words it’s the amount of product possible as.

Unit 8: Percent Yield Calculations

*Notice, kind of like the opposite of Percent Error.

Percentage Yield.

Mass Relationships in Chemical Reactions Chapter 3.

 All stoichiometry problems start with a balanced equation.  You must check for this!  If it is not balanced, BALANCE IT!

April 7, 2014 Today: Stoichiometry and % Yield. Percent Yield Remember, stoichiometry is used to tell you how much product you can form from X amount.

Theoretical, Actual, and Percent Yield Problems Example 1.

Objectives To understand the concept of limiting reactants

Limiting Reactants and Percent Yield

II. Limiting Reactants Stoichiometry – 3.7. A. Limiting Reactants b Available Ingredients 4 slices of bread 1 jar of peanut butter 1/2 jar of jelly b.

II. Stoichiometry in the Real World Stoichiometry – Ch. 11.

Chapter 9 – STOICHIOMETRY The MATH of a CHEMICAL REACTION.

Chapter 9 Chemical Quantities. Copyright © Houghton Mifflin Company. All rights reserved. 9 | 2 Information Given by the Chemical Equation Balanced equations.

The Mole & Stoichiometry!

PERCENT YIELD tells you the efficiency of a reaction tells you the efficiency of a reaction formula: formula: % yield = actual yield x 100 theoretical.

Stoichiometry: A calculation based on a balanced equation. Granada Hills Charter High School.

Stoichiometry Section 1 – Introduction to Stoichiometry, and Quantitative Relationships of Chemical Formulas Section 2 – Mathematics of Chemical Equations.

Stoichiometry: Percent Yield. What We Know You now know how to calculate the amount of product formed when specified amounts of reactants are mixed together.

PERCENT YIELD. Percent Yield Percent yield is the ratio of actual yield of an experiment to theoretical yield. To find percent yield, you divide the actual.

Chapter 9, section 3, part 2 Percent Yield. Why percent yield?  Usually, not all the product possible is actually formed.  theoretical yield  maximum.

Percent Yield. Definitions The theoretical yield is the maximum amount of product that could be made from the reactants. The actual yield is the amount.

Limiting Reactants & Percent Yield. Definitions  Limiting Reactant - completely consumed in the reaction and determines the amount of product formed.

Actual and Percent Yields So far when we have been talking about reactions we have been talking about 100% of the (limiting) reactant becoming a product.

Percentage Yield.

Chemistry in Life  You have a future job working for Consumer Reports  Testing advertising claims  An antacid company claims  Neutralizes ten times.

Limiting Reactants, Theoretical Yield, and % Yield.

Welcome: 3/10/14 Answer the following question: CaCO 3  CaO + CO 2 How many grams of CO 2 can be made from g of CaCO 3 ?

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

 Calculate empirical formula from mass percent :  Find the molecular formula of a compound has 20 % H, 80 % C, if its Mw = 30 g/mol.

SOL Review 6 Stoichiometry. Consider: 4NH 3 + 5O 2  6H 2 O + 4NO Many conversion factors exist: 4 NH 3 6 H 2 04NO 5O 2 (and others) 5 O 2 4 NO4 NH 3.

Molecular Formulas. 2 A molecular formula is equal or a multiple of its empirical formula has a molar mass that is the product of the empirical formula.

Bell Ringer Jan. 26 Balance the equation: Fe2O3 + Cl2  FeCl3 + O2

Limiting Reactant Stoichiometry

What percent is 8 of 20? If a reaction made 50. g of product, but was supposed to produce 75. g, what was the percent produced? 8 20 x 100 = 40% 50.

Percent Yield Unit 8 Lesson 3.

Percent Yield A batting average is a measure of how often a batter gets a hit as a percentage of how many times he tries. In chemistry, the percent yield.

Information Given by Chemical Equations

Percent Yield Unit 8 Lesson 3.

PERCENT YIELD Unit 8 Lesson 2.

Percent Yield Unit 7 Lesson 3.

Presentation transcript:

Stoichiometry and the Math of Equations Part 4: Percent Yield 1

Objectives Explain that the final answer to an excess-limiting problem is the theoretical amount of product made Use this knowledge and experimental data to calculate the percentage yield of a reaction 2

Percent Yield The final answer to ANY excess-limiting problem is the theoretical yield of product- the amount of product predicted from the amounts of the reactants given –Represents the maximum amount of product that can be made Reality: –The theoretical yield is rarely obtained in a real laboratory setting –Side reactions consume some of the reactants or products 3

Percent Yield Percent yield - the actual yield, the amount actually obtained, is often compared to the theoretical yield as a percentage 4

Percent Yield 68.5 g of CO is reacted with 8.60 g of H 2 gas to produce methanol (CH 3 OH). If 55.7 g of methanol is actually produced, calculate the % yield of the methanol The formula for calculating percent yield is: –Actual = What you got (experimental) –Theoretical = What you should have gotten in theory (expected) 5

68.5 g of CO is reacted with 8.60 g of H 2 gas to produce methanol (CH 3 OH). If 55.7 g of methanol is actually produced, calculate the % yield of the methanol First – find the theoretical yield (do an excess-limiting problem) 68.5 g 8.60 g ? g CO + 2 H 2 → CH 3 OH 1 mole 2 mole 1 mole 6

68.5 g of CO is reacted with 8.60 g of H 2 gas to produce methanol (CH 3 OH). If 55.7 g of methanol is actually produced, calculate the % yield of the methanol Find out which one is limiting: 68.5g CO x1 mol CO x 2 mol H 2 x 2.02g H g CO 1 mol CO 1 mol H 2 = 9.88 g H 2 so H 2 is limiting 8.60g H 2 x 1 mol H 2 x 1 mol CH 3 OH x 32.0g CH 3 OH = g H 2 2 mol H 2 1 mol CH 3 OH = 68.1 g CH 3 OH 7

68.5 g of CO is reacted with 8.60 g of H 2 gas to produce methanol (CH 3 OH). If 55.7 g of methanol is actually produced, calculate the % yield of the methanol Next, find the percent yield: What we got (given in problem) What we should have gotten 8

Objectives Explain that the final answer to an excess-limiting problem is the theoretical amount of product made Use this knowledge and experimental data to calculate the percentage yield of a reaction 9