Limiting Reactants. Reactants  Products Limiting Reactant: Determines the amount of products that can be made Excess Reactant : Left over reactants.

Slides:

Advertisements

Similar presentations

Stoichiometry (Yay!).

Advertisements

Performing Calculations involving Limiting and Excess Reagents.

Limiting Reactants & Percent Yield

Stoichiometry Chapter 12.

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

Chapter 9 Stoichiometry.

Stoichiometry Introduction.

Limiting Reagent Coach Cox.

WHAT DO THE COEFFICIENTS IN A REACTION TELL US??!?!

Determining the Mole Ratio in a Chemical Reaction Chemistry 117

USING STOICHIOMETRY TO MAKE PREDICTIONS ABOUT REACTIONS Theme: Conservation Predictions % Yield Determining Limiting Reactant.

Limiting Reactants and Excess

 CHEM.B Apply the mole concept to representative particles (e.g., counting, determining mass of atoms, ions, molecules, and/or formula units). 

Stoichiometry L.

Who can propel a rocket the farthest? The best scientist will win!

Limiting Reagent u The limiting reagent is the reactant you run out of first. u The excess reagent is the one you have left over. u The limiting reagent.

Chapter 9 Stoichiometry

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

Ch. 9: Calculations from Chemical Equations

Entry Task: March 13 th- 14 th Block 1 Entry task question: Question: 1.5 grams of zinc was added with 0.5 grams of iodine to produce zinc II iodide. Calculate.

Unit 8: Percent Yield Calculations

Stoichiometry: the mass relationships between reactants and products. We will use the molar masses ( amount of grams in one mole of a element or compound)

Daily Science feb How many grams of CH4 is needed to produce 50.0 g CHCl3? CH4 + 3Cl2  CHCl3 +3HCl Lithium reacts spontaneously with bromine to produce.

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

Stoichiometry. The Basics What is stoichiometry? A method of determining the quantities of products produced in a chemical reaction or what amount of.

S TOICHIOMETRY Ch. 12 Page 352. W HAT IS “ STOICHIOMETRY ”? A way of figuring out how much of a product can be made from a given amount of reactant Based.

Percent Yield and Limiting Reactants Advanced Chemistry Ms. Grobsky.

Limiting Reagent u If you are given one dozen loaves of bread, a gallon of mustard and three pieces of salami, how many salami sandwiches can you make?

Ch. 11: Stoichiometry Sec. 11.4: 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.

Solving a Stoichiometry Problem 1.Balance the equation. 2.Convert given to moles. 3.Determine which reactant is limiting. 4.Use moles of limiting reactant.

Unit 8 Review Stoichiometry Complete on Markerboard or in your notes.

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.

Limiting Reactants and Excess What is the Limiting Reagent (Reactant)? It is the substance in a chemical reaction that runs out first. The limiting reactant.

Follow the method Let the units guide you. When nitrogen and hydrogen react, they form ammonia gas, NH 3. If 56.0 g of nitrogen are used up in the reaction,

MAYHAN Ch. 10/12 Moles to % yield Review ws DEFINE MOLE. MAYHAN HOW IS THE MOLE USED IN CHEMISTRY? A mole is 6.02 x “things” These things are any.

Percent Yield Percent Yield is the ratio of the actual yield to the theoretical yield. Percent Yield is the ratio of the actual yield to the theoretical.

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

% 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.

Section 9.3 Limiting Reactants and Percent Yield 1.Define the terms theoretical yield and actual yield. 2.Calculate percent yield 3.Identify reasons that.

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

Unit 8 Review Stoichiometry. 1. Describe how a chemist uses stoichiometry? To determine the amount of reactants needed or products formed based on the.

Stoichiometry – Ch What would be produced if two pieces of bread and a slice of salami reacted together? + ?

STOICHIOMETRY CHE 106 Chapter Limiting Reagents Problems 3.7 In almost all chemical reactions – one reactant gets used up faster than the others.

Solving a Stoichiometry Problem

Calculations from Chemical Equations

Chemistry Limiting Reactions.

Limiting Reactants and Percent Yield

Finding the Amount of Excess Reactant Left Over

STOICHIOMETRY TUTORIAL

Ch. 9: Calculations from Chemical Equations

Limiting Reactants Why Reactions Stop.

Limiting and Excess Reactants

6 Na (s) + Fe2O3 (s) ⟶ 3 Na2O3 (s) + 2 Fe (s).

Finding the Amount of Excess Reactant Left Over

Chapter 12 CHEMICAL STOICHIOMETRY

% yield = (actual yield / theoretical yield) x 100%

Mathematics of Chemical Equations

Ch. 9 Stoichiometry Stoichiometry is a branch of chemistry that deals with the mass relationships of elements in compounds and the mass relationships between.

Chapter 11 Stoichiometry

Ch. 9 Notes -- Stoichiometry

6 Na (s) + Fe2O3 (s) ⟶ 3 Na2O3 (s) + 2 Fe (s).

Percent Yield Unit 8 Lesson 3.

Percent Yield Unit 8 Lesson 3.

PERCENT YIELD Unit 8 Lesson 2.

Percent Yield Unit 7 Lesson 3.

Presentation transcript:

Limiting Reactants

Reactants  Products Limiting Reactant: Determines the amount of products that can be made Excess Reactant : Left over reactants

Identifying the Limiting Reactant Convert each reactant to grams of a product using stoichiometry The reactant that makes the least amount of products is the limiting reactant

Sample Problem Which is the limiting reactant if 25.0 grams of phosphorus reacts with 50.0 grams of oxygen? P 4 + 5O 2  P 4 O 10 P 4 is limiting

Sample Problem A 2.00 g sample of ammonia is mixed with 4.00 g of oxygen. How much NO is produced and which is the limiting reactant? 4 NH 3(g) + 5 O 2(g)  4 NO (g) + 6 H 2 O (g)

Sample Problem An alkaline battery produces energy according to the following reaction. Determine the limiting reactant if 25.0 g of Zn and 30.0 g of MnO 2 are used. What mass of Zn(OH) 2 is produced? Zn + 2MnO 2 + H 2 O  Zn(OH) 2 + Mn 2 O 3 MnO 2 is limiting

Excess Reactants The amount of excess reactants can be determined by using stoichiometry to find the amount of reactants that is needed to react with the limiting reactant.

We're not finished yet though g is the amount of ammonia that reacted, not what is left over. To find the amount of excess reactant remaining, subtract the amount that reacted from the amount in the original sample.

Yield The theoretical yield represents the maximum amount of product that can be formed from given amounts of reactants The actual yield is the amount of product that actually forms when the reaction is carried out (in the laboratory). It is considered as an experimental value.

Percent Yield A ratio of actual yield to theoretical yield

Why might percent yield be important?

Percent yield is important, because… Higher yield=less waste Less waste= lower cost for products

Percent Error: how much error there is between actual and theoretical yield

Sample Problem Aluminum hydroxide is often present in antacids to neutralize stomach acid (HCl). If 14.0 g of aluminum hydroxide is present in an antacid tablet, determine the theoretical yield of aluminum chloride produced when the tablet reacts with stomach acid. If the actual yield of aluminum chloride is 22 g, what is the percent yield? Al(OH) 3 + 3HCl  AlCl 3 + 3H 2 O

What is the percent error?