Calculating Limiting and Excess Reagents Section 5.5 SCH 3U.

Slides:

Advertisements

Similar presentations

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

Advertisements

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

Chapter 9: Chemical quantities Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor.

Calculating Limiting and Excess Reagents

Chapter 12 Stoichiometry.

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

Stoichiometry Chemistry Ms. Piela.

Limiting Reagent and Percent Yield

Limiting Reactants and Excess

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

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.

Mole Ratios in Chemical Equations

Stoichiometry Chocolate Chip Cookies!! 1 cup butter 1/2 cup white sugar 1 cup packed brown sugar 1 teaspoon vanilla extract 2 eggs 2 1/2 cups all-purpose.

and cooking with chemicals

Stoichiometry The Mole: Review A counting unit Similar to a dozen, except instead of 12, it’s 602,000,000,000,000,000,000, X (in scientific.

Chapter 12 Stoichiometry. Another Analogy: (let’s get off the bike for a while and bake a cake!)  Let’s say you want to bake a cake. Here’s a recipe:

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

Chapter 12 Stoichiometry.

Chapter 11 Stoichiometry.

Stoichiometry Calculating Masses of Reactants and Products.

Stoichiometry Chemistry IH: Chapter 9 Stoichiometry The method of measuring amounts of substances and relating them to each other.

Stoichiometry Chapters 7 and 9.

C.7 (notes) – C.8 (practice) In which you will learn about… In which you will learn about… Mole ratios Mole ratios stoichiometry stoichiometry.

Stoichiometry mass and amount relationships between reactants and products in a chemical reaction.

Stoichiometry * The key is a balanced equation and reading the equation in terms of…Coefficients! The branch of chemistry that deals with the mass relationships.

MOLE-MOLE AND MASS-MASS CONVERSIONS Stoichiometry 1.

Stoichiometry Chemistry I: Chapter 9 Molar Mass of Compounds The molar mass (MM) of a compound is determined the same way, except now you add up all.

Chapter 9 Section 2. Chocolate chip cookies 1 c. butter ½ c. granulated sugar 1 c. brown sugar 1 tsp. vanilla 2 eggs 2 ½ c. flour 1 tsp. baking soda 1.

Start-Up What is the molar mass for Calcium hydroxide? A g/mol B g/mol C g/mol D. 27 g/mol.

Chp 9: Stoichiometry Chocolate Chip Cookies!! 1 cup butter 1/2 cup white sugar 1 cup packed brown sugar 1 teaspoon vanilla extract 2 eggs 2 1/2 cups.

Stoichiometry Topic – Chocolate Chip Cookies!! 1 cup butter 1/2 cup white sugar 1 cup packed brown sugar 1 teaspoon vanilla extract 2 eggs.

Stoichiometry Chapter 12

Section 9-2: Ideal Stoichiometric Calculations

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 Mole: Review A counting unit A counting unit Similar to a dozen, except instead of 12, it’s 602,000,000,000,000,000,000,000 Similar.

The Mole & Stoichiometry!

3.8 Stoichiometry & Mole Ratios. Recipe for 24 brownies 1cup flour 4oz. chocolate 2 eggs 1cup sugar 1 cup flour + 4 oz. chocolate + 2 eggs + 1 cup sugar.

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

Stoichiometry A chemical equation shows the reactants (left side) and products (right side) in a chemical reaction. A balanced equation shows, in terms.

The Limiting Reactant Chemistry 11 Ms. McGrath. The Limiting Reactant The coefficients of a balanced chemical chemical equation gives the mole ratio of.

It’s time to learn about.... Stoichiometry Stoichiometry : Mole Ratios to Determining Grams of Product At the conclusion of our time together, you should.

Stoichiometry and cooking with chemicals.  Interpret a balanced equation in terms of moles, mass, and volume of gases.  Solve mole-mole problems given.

Ch. 9 Notes -- Stoichiometry Stoichiometry refers to the calculations of chemical quantities from __________________ chemical equations. Interpreting Everyday.

Chapter 9 Stoichiometry 9.3 Limiting reagent and percent yield.

Can’t directly measure moles Measure units related to moles: –Mass (molar mass) –Number of particles (6.02 x ) –Liters of gas (22.4 Liters at STP)

Stoichiometry. Do Now A recipe calls for one cup of milk and three eggs per serving. You quadruple the recipe because you are expecting guests. How much.

Chapter Three Mass Relationships in Chemical Reactions.

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

Stoichiometry  the calculations of quantities in chemical reactions  “stoichio” = elements  “metry” = to measure.

Chapter 9A Notes Stoichiometry

MASS - MASS STOICHIOMETRY

Unit 4: Stoichiometry Stoichiometry.

Chemical Stoichiometry

Limiting Reactant/Reagent Problems

Unit 4: Chemical Equations and Stoichiometry

Ch. 9 Notes -- Stoichiometry

Stoichiometry mass and amount relationships between reactants and products in a chemical reaction.

Unit 4: Chemical Equations and Stoichiometry

Stoichiometry Chapter 12.

Stoichiometry & Limiting Reactants

Unit 5: Stoichiometry Stoichiometry.

Chemical Calculations

Chapter 9- Stoichiometry:

Calculation of Chemical Quantities

Notes Ch Limiting Reagent and Percent Yield

Reaction Stoichiometry

Presentation transcript:

Calculating Limiting and Excess Reagents Section 5.5 SCH 3U

The Mole Ratio The quantities of substances that react in a chemical reaction are determined by the mole ratio given by the balanced chemical equation but, in the real world, it is less likely for the reactants to be in the mole ratios given by the equation – WHY??

The Answer In nature, compounds are found in random quantities In labs / industry, we might want to ensure that one reactant is completely used up

In any chemical reaction, one reactant is always present in EXCESS - in other words: the reagent that is not completely used up in the reaction there will be some left over at the end of the reaction in order to provide a reagent in excess, chemists add 10% to the mass required The Excess Reagent

The other reactant is LIMITING - in other words: it is completely used up in the reaction the reagent in a chemical reaction that limits the amount of product that is able to form The Limiting Reagent

Kitchen Stoichiometry – an analogy A recipe to make 30 candies requires the following: 2 cups water 5 cups sugar 1 cup strawberries Equation 2 c water + 5 c sugar + 1 c strawberries  30 candies

a. If you were given 10 cups of water, 10 cups of sugar and 10 cups of strawberries, which ingredient would limit the amount of candies being made? Which reagent is in excess? Questions:

b. How many candies can you make with the ingredients given in part a? Questions:

c. How much of the excess reagents will be left over? Questions:

Lithium nitride reacts with water to produce ammonia gas and lithium hydroxide. If 4.5 g of lithium nitride and 5.8 g of water is available: a. How much ammonia gas (in grams) can be produced? Step 1: Write a balanced chemical equation. Step 2: Choose a product – pick the one that you will need to calculate the amount of (ammonia). Step 3: Determine the amount of ammonia that can be produced from each of the reactants. Step 4: Compare the amounts of product formed from the lithium nitride and from the water – the one that produces the least ammonia is the limiting reagent Example 1:

Lithium nitride reacts with water to produce ammonia gas and lithium hydroxide. If 4.5 g of lithium nitride and 5.8 g of water is available: b. How much (in grams) of the excess reagent will be left over? Li 3 N (s) + 3H 2 O (l) → 3LiOH (aq) + NH 3(g) Example 1:

Nitrogen and hydrogen react to form ammonia according to the following equation: N 2(aq) + H 2(g) → NH 3(g) If g of N 2 is to be completely used up, what is a reasonable mass of H 2 to use in the reaction? Example 2: