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.

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)

Chemical Quantities Chapter 9

Mathematics of Chemical Equations By using “mole to mole” conversions and balanced equations, we can calculate the exact amounts of substances that will.

Laboratory 08 LIMITING REACTANT LAB.

Stoichiometry Ch.10. (10-1) Stoichiometry Mass & amt relationships b/w reactants & products –Conversions b/w grams & moles Always begin w/ a balanced.

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

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 Reactants & Percent Yield

Limiting Reagent and Percent Yield

Limiting Reagents and Percent Yield

Identify the limiting reactant and calculate the mass of a product, given the reaction equation and reactant data. Include: theoretical yield, experimental.

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

Is this a balanced eq ? We only need ONE information during the reaction (reacted or produced)

12.3 Limiting Reagent and Percent Yield

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

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 1 Chapter 9 Chemical Quantities in Reactions On a space shuttle, the LiOH in the canisters removes.

STOICHIOMETRY Calculations Based on Chemical Equations.

Stoichiometry Loose Ends: Limiting Reactants, Percentage Yield, and Percentage Error.

 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.

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

Stoichiometry Chapter 9. Step 1 Balance equations and calculate Formula Mass (FM) for each reactant and product. Example: Tin (II) fluoride, SnF 2, is.

STOICHIOMETRY REVIEW ANSWERS

STOICHIOMETRY 4 Mole-Mole 4 Mole-Mass 4 Mass-Mass.

UNIT 6: STOICHIOMETRY PART 2: STOICHIOMETRY. KEY TERMS Actual yield - Amount of product was actually made in a reaction Dimensional analysis - The practice.

Objectives To understand the concept of limiting reactants

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

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

Chapter 12 Stoichiometry. 1. The part of chemistry that deals with the amount of substances involved in chemical reactions A. 3 basic steps to every stoichiometry.

Limiting Reactions and Percent Yield Calculating by moles or mass ©2011 University of Illinois Board of Trustees

Theoretical yield: amounts of product calculated from the limiting reagent. Actual yield: amount produced during the conducted experiment. Percentage.

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

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.

Limiting Reagent and Percent Yield Chapter 12.3 Page 368.

Do Now 1 Read the balanced equation below and write all possible mole ratios. 2Al 2 O 3 → 4Al(s) + 3O 2 (g)

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

Copyright©2004 by Houghton Mifflin Company. All rights reserved. 1 Introductory Chemistry: A Foundation FIFTH EDITION by Steven S. Zumdahl University of.

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.

Products Percent Yield. Theoretical Yield Maximum amount of product Calculation Balanced Equation Given mass Molar Mass Mole Ratios.

Theoretical Yield and Percent Yield Recipe says makes 3 dozen, you get 30. Your percent yield is 83.33%.

Percentage 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.

Stoichiometry Chemistry – Chapter 12.

Stoichiometry Chemistry – Chapter 12.

Chapter 9 STOICHIOMETRY

Percentage Yield.

Limiting and Excess Reactants

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

Mathematics of Chemical Equations

Calculations Based on Chemical Equations

Stoichiometry Chapter 12.

Unit 5 STOICHIOMETRY.

Information Given by Chemical Equations

Percentage Yield.

Quiz 02/18/2016 Foothill Chemistry.

Yield-noun: Performance, production, product. Harvest, crop.

Percentage Yields.

Chapter 11 Review.

Stoichiometry Preparation for College Chemistry Luis Avila

Presentation transcript:

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. However in real- life most of the time some of the reactants do not react so our theoretical (if 100% of reactants become product) yield is different from our actual yield. We can express this difference as a percentage to see if a reaction would be viable.

LiOH + KCl  KOH + LiCl If I start this reaction with 20g of LiOH, what mass of LiCl should I get? If I actually get 6g of LiCl, what is my percent yield? Step 1: Write a balanced equation Step 2: Calculate the number of moles of reactant 1 mole LiOH = 24g 20g = 20/24 moles = 0.83 moles

Step 3: Use mole ratios to calculate the mass of product 1 mole LiOH : 1 mole LiCl 0.83 moles LiOH : 0.83 moles LiCl 1 mole LiCl = 42.5g 0.83 moles = 42.5 x 0.83 = 35.28g Theoretical Yield Step 4: Calculate percent yield using the formula % yield = Actual yield Theoretical yield X X 100 = 17% yield From question From step 3