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

Slides:

Advertisements

Similar presentations

Stoichiometry: The study of quantitative measurements in chemical formulas and reactions Chemistry – Mrs. Cameron.

Advertisements

Chapter 5 Chemical Reactions

HONORS CHEMISTRY Feb 27, Brain Teaser Cu + 2 AgNO 3  2 Ag + Cu(NO 3 ) 2 – How many moles of silver are produced when 25 grams of silver nitrate.

CHEMISTRY February 13, 2012.

Stoichiometry Chemistry Ms. Piela.

Limiting Reagent and Percent Yield

Percent Yield and Limiting Reactants

Section 12.3: Limiting Reagent and Percent Yield

Limiting Reactants & Percent Yield

Reaction Stoichiometry.

Limiting Reagents and Percent Yield

Starter S moles NaC 2 H 3 O 2 are used in a reaction. How many grams is that?

NOTES: 12.3 – Limiting Reagent & Percent Yield

Chapter 9 – Review Stoichiometry

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.

Sodium Bicarbonate Decomposition Edward A. Mottel Department of Chemistry Rose-Hulman Institute of Technology.

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

Brought to you by Coach Cox PERCENT YIELD. WHAT IS PERCENT YIELD? Theoretical Yield – the maximum amount of product that can be produced from a given.

Chemistry 11 Stoichiometry Reality II: Percent Yield.

PERCENT YIELD This is used A LOT in ORGANIC CHEMISTRY.

Percentage Yield of a Chemical Reaction. Let’s look at your last Chemistry Test You scored 32/40. What’s your % grade? (32/40) * 100% = 80% What is the.

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.

Percent Yield Theoretical Yield Actual Yield. Theoretical Yield The maximum amount of product that can be formed from given amounts of reactants The amount.

Stoichiopardy Holy Moley Do the 2 or 3 step Random Limit my Percent Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400 Q $500 Final Chempardy.

Stoichiometry Jeopardy Percen t Yield Limiting Reactan ts “Stoiche d” About Chemist ry Q $100 Q $200 Q $300 Q $400 Q $ Q $100 Q $200 Q $300 Q $400.

1 Chapter 9-Stoichiometry Stoichiometry – measures and calculates amounts of chemicals in a reaction. A.Mole/Mole Problems Coefficients: Show # of molecules.

Stoichiopardy Holy Moley Do the 2 or 3 step Star Wars Limit my Percent Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400 Q $500 Final Chempardy.

Percent Yield Section 12.4.

Percentage Yield.

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.

Test Review Chemical Reactions and Stoichiometry.

Stoichiometry. Information Given by the Chemical Equation  The coefficients in the balanced chemical equation show the molecules and mole ratio of the.

Limiting Reactants and Percent Yield

Stoichiometry. What Is It? Branch of chemistry that shows the relationships among reactants and products in a chemical reaction Equations must be balanced.

Stoichiometry Chapter 12

Section 11.3: Stoichiometry of Gases Apply Gay-Lussac and Avogadro’s discoveries to the stoichiometry of reactions involving gases… For gaseous reactants.

Chapter 12 Stoichiometr y. STOY-KEE-AHM-EH-TREE Founded by Jeremias Richter, a German chemist Greek orgin: stoikheion: element & metron: measure Stoichiometry—the.

Stoichiometry! The heart of chemistry. The Mole The mole is the SI unit chemists use to represent an amount of substance. 1 mole of any substance = 6.02.

Percentage Yield Chemistry 11 Ms. McGrath.

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.

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.

Chemistry 521 Chapter 4.  Stoichiometry is the study of the relative quantities of reactants and products in chemical reactions.  Ex:  Two hydrogen.

Reaction Yield. Theoretical vs Actual Yield Theoretical yield is the maximum amount of product that can be produced from a given amount of reactant Calculated.

Percentage Yield.

 How far away you are from a theoretical or “actual” value.

% Yield. % yield = actual yield _ x 100 theoretical yield Actual yield is found in a lab or you must be given this value Theoretical yield is amount of.

Stoichiometry Notes (Chapter 12). Review of Molar Mass Recall that the molar mass of a compound is the mass, in grams, of one mole of that compound.

Students type their answers here

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.

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

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.

Challenge Problem When nitrogen and hydrogen react, they form ammonia gas, which has the formula NH 3. If 56.0 g of nitrogen are used up in the reaction,

Mass-Mass Conversions 56.0 g N 2 x g N 2 g NH = 1904 = When nitrogen and hydrogen react, they form ammonia gas, which has the formula.

Let’s talk… mole to mole

Yield Amount of Products 1.

7.3 Percentage Yield.

Excess Reactant and Percent Yield

Chapter 12 Review.

Chapter 12 Review.

Reaction Yield.

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.

Chapter 7: 7.3 Reaction Yields

Chapter 7 7.3: Percentage Yield.

Calcium carbonate, found in limestone and marble, reacts with hydrochloric acid to form calcium chloride, carbon dioxide and water. What mass of CO2 could.

Presentation transcript:

Percentage Yield Chemistry 11 Ms. McGrath

Percentage Yield In this last unit, we will earn how chemists calculate a percentage that will determine how successful a reaction will be, ie how much product will be produced.

Percentage Yield The amount of product that is predicted by stoichiometry is called the theoretical yield. This predicted product is not always the same as the amount of product that is actually obtained during the reaction. The amount of product obtained in an experiment is called the actual yield.

Percentage Yield A reduced yield may be caused by a competing reaction – a reaction that occurs at the same time as the principal reaction. For example, phosphorus reacts with chlorine to produce phosphorus trichloride. Phosphorus trichloride then may react with chlorine to form phosphorus pentachloride.

Percentage Yield There are certain reasons why the percentage yield may be off. What do you think these may be?

Percentage Yield Some causes are: 1.competing reactions; 2.poor experimental technique; 3.impure reactants; 4.faulty measuring devices.

Percentage Yield The percentage yield of a chemical reaction compares the mass of a product obtained by the experiment (the actual yield) with the mass of the product determined by stoichiometry calculations (the theoretical yield).

Calculating Percentage Yield Ammonia can be prepared by reacting nitrogen gas, taken from the atmosphere, with hydrogen gas. When 7.5 g of nitrogen reacts with sufficient hydrogen, the theoretical yield of ammonia is 9.10 g. If 1.72 g of ammonia is obtained by experiment, what is the percent yield of the reaction?

Calculating Percentage Yield Actual yield = 1.72 g Theoretical yield = 9.10 g Percentage yield: = 1.72 g x 100 % 9.10 g = 18.9 %

Predicting actual yield based on percentage yield Calcium carbonate can be thermally decomposed to calcium oxide and carbon dioxide. CaCO 3(s) -> CaO (s) + CO 2(g) Under certain conditions, this reaction proceeds with a 92.4 % yield of calcium oxide. How many grams of calcium oxide can the chemist expect to obtain if 12.4 g of calcium carbonate is heated?