Percent Yield.

Slides:

Advertisements

Similar presentations

Stoichiometry Ratios The stoichiometric coefficients in a balanced chemical reaction can be used to determine the mole relationships between any combination.

Advertisements

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

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.

Section 3: Limiting Reactants

Limiting Reactants and Percent Yields

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

WE CANNOT SOLVE OUR PROBLEMS WITH THE SAME THINKING WE USED WHEN WE CREATED THEM. –Einstein-

Review Answers with step-by-step examples

Chemistry I Unit 8: Stoichiometry Text Questions from

Chemistry 11 Stoichiometry Reality II: Percent Yield.

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

The general steps for finding PERCENT YIELD : * Write the balanced chemical equation * Find the limiting reactant * Find the theoretical yield (what you.

Stoichiometry Chapter 12. Stoichiometry STOY-KEE-AHM-EH-TREE – Founded by Jeremias Richter, a German chemist – Greek orgin stoikheion – element & metron.

Chapter 12 Stoichiometry. What is Stoichiometry? Stoichiometry is at the heart of the production of many things you use in your daily life. Soap, tires,

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

Percent Yield Section 12.4.

Theoretical, Actual, and Percent Yield Problems Example 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.

Ch. 11: Stoichiometry Sec. 11.4: Percent Yield.

Stoichiometry Chapter 12. Stoichiometry STOY-KEE-AHM-EH-TREE – Founded by Jeremias Richter, a German chemist – Greek orgin stoikheion – element & metron.

Percentage Yield. Success Criteria Be able to explain the difference between actual and theoretical yield. Be able to calculate the percentage yield of.

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

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.

Limiting Reagent and Percent Yield Chapter 12.3 Page 368.

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

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.

Percent Yield. Percent yield describes the efficiency of a chemical reaction 100 free throws Theoretically… Actually…

NIS – CHEMISTRY Lecture 65 Percent Yield Ozgur Unal 1.

Stoichiometry Chapter 9 Percent Yield Stoich ppt _5 Percent Yield.

Jeopardy $100 Stoich Vocab Stoich Calculations Stoich True/False Percent Yield Limiting Reactants $200 $300 $400 $500 $400 $300 $200 $100 $500 $400 $300.

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 ?

Percent yield is a measure of the efficiency of a chemical reaction. Section 4: Percent Yield K What I Know W What I Want to Find Out L What I Learned.

Minds On… The reaction of potassium tetrachloroplatinate II (K 2 PtCl 4 ) with potassium iodide (KI) is used to make the cancer drug Cisplatin. Given that.

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

Unit 6: Limiting Reactants and Percent Yield Chapter 11.3 and 11.4.

1 1)Write correct chemical formulas, know types of reactions and write a balanced equation!!! 2)a) Convert g, L or # or particles to mole and b) use mole.

Stoichiometry Pronounced: Stoy-kee-AHM-uh-tree. What is stoichiometry? Its math that helps us to see the relationship between what is used and formed.

Let’s look at the butane reaction once more: 2C 4 H O 2 → 8CO H 2 O What do the coefficients represent? Stoichiometry is the use of these.

Unit 10 Stoichiometry.

Stoichiometry Chapter 11.

Stoichiometry Chemistry – Chapter 12.

Stoichiometry From the Greek words “stoicheion” meaning “element”

DO NOW!!! Back of Worksheet!

Stoichiometry Chemistry – Chapter 12.

Percent Yield in a Chemical Reaction.

UNIT 9 STOICHIOMETRY.

9.5 – NOTES Limiting Reactants and Percent Yield

October 25 & Ms. Boon Chemistry

Percentage Yield.

Percent Yield Theoretical Yield Actual Yield

Reaction Yield.

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

Lecture 4.5 – Percent Yield

Chapter 12 Stoichiometry.

Stoichiometry Chapter 12.

Reaction Yield.

Information Given by Chemical Equations

Chemical Calculations

Percentage Yield.

Ch 9 Stoichiometry How does this apply to everyday life?

Limiting Reactants and Percent Yield

Quiz 02/18/2016 Foothill Chemistry.

Cu (s) + 2AgNO3(aq) → Cu(NO3)2 (aq) + 2Ag(s)

7.1 Describing Reactions In a chemical reaction, the substances that undergo change are called reactants. The new substances formed as a result of that.

Percentage Yields.

Presentation transcript:

Percent Yield

Why is it important? Chemical reactions rarely produce the predicted amount of product. Most rxns produce less than the expected amount of product liquid reactants/products stick to glassware evaporation product is lost during purification other unexpected products are formed (side products)

Actual versus Theoretical Yield Theoretical yield: the calculated yield based on the balanced chemical equation Actual yield: the amount actually produced when the reaction is carried out in an experiment In the problem you will almost always be given the actual yield. This is the result of the experiment, so you don’t want to have to go complete an experiment to work a problem. If you are not given actual yield, then you must be given the percent yield and asked to find actual yield.

What does it tell me? % yield is a measure of how efficient the reaction was

How to calculate % yield % yield = actual (measured) yield/theoretical (predicted) yield x 100

Determining % yield step 1: calculate the theoretical yield step 2: measure the actual yield step 3: actual/theoretical x 100

Example K2CrO4 + 2 AgNO3  Ag2CrO4 + 2 KNO3 If 0.500 g AgNO3 was used and the actual yield of Ag2CrO4 was 0.455 g, what is the percent yield?

Calculating % yield K2CrO4 + 2 AgNO3  Ag2CrO4 + 2 KNO3 step 1: calculate the theoretical yield: determine the molar mass AgNO3 = 107.87 + 14.01 + 3(16) = 169.9 Ag2CrO4 = 2(107.87) + 52 + 4(16) = 331.7

Calculating % yield K2CrO4 + 2 AgNO3  Ag2CrO4 + 2 KNO3 step 1: calculate the theoretical yield given 0.500 g silver nitrate: K2CrO4 + 2 AgNO3  Ag2CrO4 + 2 KNO3 0.500 g AgNO3 (331.7 g) (1 mol) Ag2CrO4 (169.9 g) (2 mol) AgNO3 (0.500) (331.7) (1) = 0.488 g Ag2CrO4 (169.9) (2)

Calculating % yield step 2: measure the actual yield 0.455 g Ag2CrO4 step 3: actual/theoretical x 100 0.455 g Ag2CrO4 x 100 0.488 g Ag2CrO4 % yield = 93.2%

Importance of % Yield A chemist must balance cost, % yield and the speed of the rxn to minimize cost and comply with environmental standards.