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.

Slides:

Advertisements

Similar presentations

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

Advertisements

Limiting Reactants & Percent Yield

Limiting Reactant & Percent Yield Notes Background Knowledge Check Label the reactant(s) and product(s) in the following reaction: 2 Mg + O 2  2MgO.

Chemical Quantities In Reactions

Chemical Quantities Chapter 9

Stoichiometry Chapter 12.

Chemical Reactions Unit

Limiting Reactants Very rare that reactants are present in the same ratio that they are used in the rxn. This means one reactant will run out first. This.

Stoichiometry Introduction.

Limiting Reactant Percent Yield. Consider the following reaction 2 H 2 + O 2  2 H 2 O.

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

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.

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

Percent Yield. Yield u The amount of product made in a chemical reaction. u There are three types u Actual yield- what you get in the lab when the chemicals.

Stoichiometry Chapter 3. Atomic Mass Atoms are so small, it is difficult to weigh in grams (Use atomic mass units) Atomic mass is a weighted average of.

Section 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.

Unit 6 Stochiometry. Information Given by Chemical Equations Example: CO (g) + 2H 2(g)  CH 3 OH (l) The numbers we put in front of each element is called.

Chemistry 11 Stoichiometry Reality II: Percent Yield.

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

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.

Stoichiometry – Chemical Quantities Notes Stoichiometry Stoichiometry – Study of quantitative relationships that can be derived from chemical formulas.

Reaction Stoichiometry.   Deals with the mass relationships that exist between reactants and product  In this type of chemistry, a quantity is given,

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

STOICHIOMETRY Calculations Based on Chemical Equations.

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

Percent Yield Section 12.4.

Chapter 3 Stoichiometry Deals with quantities of materials consumed and produced in chemical reactions.

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.

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.

Chapter 9 STOICHIOMETRY. What’s it mean? Greek stoikheion, meaning elementelement metron, meaning measuremeasure In English….chemical recipe.

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

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

Objectives To understand the concept of limiting reactants

Limiting Reactants and Percent Yield

Stoichiometry & Percent Yield Practice 2 Al + 6 HCl  2 AlCl H 2 95 g of hydrochloric acid are reacted with excess aluminum producing 2.2 g of hydrogen.

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

Percentage Yield Chemistry 11 Ms. McGrath.

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

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. “yield—” the amount of product actually made through a chemical reaction. Why is this value important? Theoretical yield— calculated amount.

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

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

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.

Chapter 9 Chemical Quantities. 2 cup brownie mix + ½ c H 2 O + ¼c oil + 2 eggs  24 brownies What other items require a recipe? What do the numbers in.

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.

1 Percent Yield. 2 Theoretical, Actual, and Percent Yield Theoretical yield The maximum amount of product calculated using the balanced equation. Actual.

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

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

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,

Actual Yield The amount of product formed from the actual chemical reaction and it is usually less than the theoretical yield.

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

Stoichiometry and the Mole

Theoretical Yield The maximum amount of product that can be produced from a given amount of reactant.

Theoretical Yield.

Reaction Yield.

Chapter 7: 7.3 Reaction Yields

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

Information Given by Chemical Equations

Thanks to Piedra Vista High, School, Farmington, NM

Percent Yield Unit 7 Lesson 3.

Presentation transcript:

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. You know that the amount of product formed is controlled by the limiting reactant. –Products stop forming when the limiting reactant runs out

Theoretical Yield The amount of product formed in these calculations is called the theoretical yield. Theoretical yield is the amount of a given product that can be formed when the limiting reactant is completely consumed.

Theoretical Yield In stoichiometry problems you are predicting the maximum amount of product that can be produced. In reality, the maximum amount is rarely obtained. –This could be due to side reactions, human error, or various other causes.

Actual Yield The amount of product you actually obtain in a chemical reaction is called the actual yield. This is the amount you measure in the lab, not what you calculated in a stoichiometry problem.

Percent Yield Percent yield is the actual yield of a product as a percentage of the theoretical yield. Gives you a comparison between what you thought would be produced (theoretical yield) and what actually was produced (actual yield).

Percent Yield Actual Yield / Theoretical Yield x 100 = Percent Yield Divide the actual yield by the theoretical yield and multiply by 100 to get the percent yield.

Practice Problem Methanol (CH 3 OH) can be produced by the reaction between carbon monoxide and hydrogen. Suppose 6.85 x 10 4 g of carbon monoxide is reacted with 8.60 x 10 3 g of hydrogen. What is the theoretical yield of methanol? If 3.57 x 10 4 g of methanol is actually produced, what is the percent yield of methanol?

Practice Problem Titanium (IV) oxide is a white compound used as a coloring pigment. In fact, the pages in your textbook are white because of the presence of this compound in the paper. Solid titanium (IV) oxide can be prepared be reacting gaseous titanium (IV) chloride with oxygen gas. A second product of this reaction is chlorine gas. If 6.71 x 10 3 g of titanium (IV) chloride reacts with 2.45 x 10 3 g of oxygen, what is the mass of titanium (IV) oxide that can form? If the percent yield of titanium (IV) oxide is 75%, what mass is actually formed?