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

Slides:

Advertisements

Similar presentations

Chemistry 12.3 “Limiting Reagent and Percent Yield”

Advertisements

Laboratory 08 LIMITING REACTANT LAB.

Percent Yield and Limiting Reactants

Limiting Reactants and Percent Yields

Limiting Reactants & Percent Yield

Percentage Yield Chemistry 11 Ms. McGrath. Percentage Yield In this last unit, we will earn how chemists calculate a percentage that will determine how.

Section Limiting Reagent and Percent Yield

Limiting Reagents Excess Reagents Percent yield

Stoichiometry of Chemical Equations and Formulas.

Limiting Reagents Determine the mass of P 4 O 10 formed if 25g P 4 and 50g O 2 are combined. P 4 + 5O 2  P 4 O 10 What is the given? We have to find the.

Limiting Reagent and Percent Yield

Limiting and Excess Reagents

Limiting Reagents and Percent Yield

Limiting and Excess Reagents

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.

12.3 Limiting Reagent and Percent Yield

STOICHIOMETRY.  Stoichiometry is the science of using balanced chemical equations to determine exact amounts of chemicals needed or produced in a chemical.

Chemistry 11 Stoichiometry Reality II: Percent Yield.

PERCENT YIELD This is used A LOT in ORGANIC CHEMISTRY.

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.

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

Calculations Using Chemical Equations Chapter 10.

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

Things you must KNOW and what to expect  Things you must KNOW  You must KNOW your polyatomics  You must KNOW how to write a balanced formula  You have.

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.

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.

Percent Yield Section Percent Yield Often when reactions are actually carried out in the lab, there is a difference between the amount of product.

Balancing Equations and Stoichiometry. Chemical Equations Terms: (s) = solid (l) = liquid (g) = gas  = heat (aq) = aqueous solution.

Objectives To understand the concept of limiting reactants

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

Percentage Yield Chemistry 11 Ms. McGrath.

1.3 Reacting Masses and Volumes Stoichiometry, Limiting & Excess Reactants, Theoretical & Percent Yields Mrs. Page - IB SL Chemistry

Reaction Stoichiometry. Objectives Understand the concept of stoichiometry. Be able to make mass-to-mass stoichiometric calculations.

Stoichiometry Warmup I have 1 mole of CO 2 gas at STP. How many grams of CO 2 do I have? How many Liters of CO 2 do I have? How many molecules of CO 2.

Limiting reagents In lab a reaction is rarely carried out with exactly the required amounts of each reactant. In lab a reaction is rarely carried out with.

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.

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

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

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.

Limiting Reactants Unit 7 1. Limiting Reactants 2.

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

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.

Yield Amount of Products 1.

Combustion Analysis A g sample composed of C, H, N is burned to produce g CO2 and g H2O Assume all C in the sample is converted to CO2.

Chapter 9 STOICHIOMETRY

Percent Yield actual yield % yield = x 100 theoretical yield

Percentage Yield.

7.5 Percentage Yield.

Combustion Analysis A g sample composed of C, H, N is burned to produce g CO2 and g H2O Assume all C in the sample is converted to CO2.

Percentage Yield.

Percentage Yield.

Chemical Reactions and Stoichiometry

Limiting and Excess Reactants

Theoretical Yield.

Percentage Yield.

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

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

Stoichiometry Chapter 12.

Limiting Reagent and Percent Yield

Percentage Yield.

Chemical Calculations

Percentage Yield.

Chemical Reactions Limiting Reagent.

Chapter 11: Stoichiometry

Quiz 02/18/2016 Foothill Chemistry.

Presentation transcript:

Theoretical yield: amounts of product calculated from the limiting reagent. Actual yield: amount produced during the conducted experiment. Percentage yield: ratio of actual to theoretical yield expressed in percentage. actual yield theoretical yield percent yield = x 100

Reactions are influenced by "external" factors which effect the amount of yield produced: 1.Concentration 2.State (s, l, g, aq) 3.Temperature 4.Pressure (of gas reactants) 5.Human error Poor recovery Impurities in reactants Miscalculation A side reaction occurs

5.00 g of KClO 3 is heated and decomposes to yield 1.78 g of O 2. What is the % yield? 3 mole O 2 2 mole KClO 3 1 mole g 5.00 g KClO g O 2 1 mole O 2 = 1.96 g O 2 2 KClO 3  2 KCl + 3 O 2 actual yield theoretical yield percent yield = x g 1.96 g 90.8 %

How much O 2 would be produced if the percentage yield was 78.5%? Ac. yield Th. yield % yield = x 100 = Ac. yield 1.53 g 1.96 g 78.5 % =

What is the % yield if 58 g H 2 O are produced by combining 60.0 g O 2 and 7.0 g H 2 ? 2 mole H 2 1 mole O g O g O g H 2 1 mole H 2 O 2 (g) + 2 H 2 (g) 2 H 2 O (g) = 7.5 g H 2 H 2 - limiting reactant, O 2 - excess reactant

2 mole H 2 O 2 mole H 2 1 mole H g H g H g 1 mole = 63 g H 2 O produced actual yield theoretical yield percent yield = x g 63 g 92 %