LIMITING REAGENT. LIMITING & EXCESS REACTANT Before the reaction has started After the reaction is complete CO (g) + 2 H 2 (g) CH 3 OH (g)

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

When a lump of zinc is added into copper sulfate solution, the two slowly react to produce very small dark copper granules and zinc sulfate solution.

Limiting Reactants and Stoichiometry

Calculations from Equations Chapter 9

II. Stoichiometry in the Real World Limiting Reagents and % yield (p ) Stoichiometry – Ch. 12.

Chapter 9 - Section 3 Suggested Reading: Pages

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.

Stoichiometry Chapter 12.

Limiting Reactions and Percentage Yield

1 Calculations From Chemical Equations Chapter 9 Hein and Arena Version 1.1.

Stoichiometry Hein and Arena Version 1.1

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

1. 2 A Short Review 3 The mole weight of an element is its atomic mass in grams. It contains 6.02 x atoms (Avogadro’s number) of the element.

Limiting Reactant.

Limiting reactant.

Calculating Reacting Masses

Stoichiometry TJ Bautista, Sean Higgins, Joanna Lee Period 6.

9.3 Notes Limiting reagents.

Unit 3: Chemical Equations and Stoichiometry

Stoichiometry Board Relay

IB Chemistry Topics for Test #1. General definitions  Mole  Homogeneous mixture  Heterogeneous mixture  Pure Substances  Compounds  Chemical.

Foundations of College Chemistry, 14 th Ed. Morris Hein and Susan Arena Accurate measurement and dosage calculations are critical in dispensing medicine.

Test Review Chemical Reactions and Stoichiometry.

Calculating Yield L.O: To be able to calculate yield for chemical reactions.

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

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

1 Chapter 8 Quantities in Chemical Reactions Tro, 2 nd ed.

In the reaction: CH 4 + 2O 2  CO 2 + 2H 2 O How many moles of CH 4 react with 6 moles of O 2 ? A.2 moles B.4 moles C.3 moles D.1 mole.

Day SOLVE: 1.5e24 molecules of SO 2 = ____ grams of SO 2 ? S 2 + 2O 2  2SO 2 And how many moles of S 2 ?

Stoichiometry-the study of the ____________ relationships between the amounts of __________ used and the amounts of __________ formed during a __________.

Recall: A limiting reagent is the reactant whose entities are completely consumed in a reaction. It is the one that runs out first, and as a result, stops.

4.5 Precipitation Reactions

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

Stoichiometry: Limiting and Excess Reagents. Bon Appetite Suppose you are a chef preparing French toast for a group of people. You make French toast the.

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.

Net Ionic 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.

Mass-Mass Stoichiometry If the mass of any reactant or product is known for a chemical reaction, it is possible to calculate the mass of the other reactants.

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.

WARM UP 1.Given the following reaction…… Ba(NO 3 ) 2(aq) + Na 2 CO 3(aq)  BaCO 3(s) + 2 NaNO 3(aq) Calculate the yield of sodium nitrate when you start.

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

Raider Rev Up Calculate moles in g of HgS (mercury II sulfide) MAR

Stoichiometry Chapter 9. Do Now Balance the equation Al + HCl → H 2 + AlCl 3 1.How many moles of HCl are required to produce 2 moles of AlCl 3 ? 2.How.

Stoich Review. Particles in 10.5 mols of Ammonium Nitrate.

K sp and the Solubility Product Constant. K sp The Solubility Product Constant The study of __________ _________ compounds.

Mass Relationships in Chemical Reactions Chapter 3.

1 Question of the Day A solution containing 3.50 g sodium phosphate is mixed with a solution containing 6.40 g barium nitrate. After the reaction is complete,

Stoichiometry Introduction to Chemistry. Stoichiometry Example: 2H 2 + O 2 → 2H 2 O Equivalencies: 2 mol H 2 for every 1 mol O 2 2 mol H 2 for every 2.

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

Limiting Reactants and Stoichiometry

Balanced Equations 2H2 + O2  2H2O

9.2 Solution Stoichiometry

Here is a helping hand with some of the new material on Molarity:

Calculations from Equations Chapter 9

Finding the Amount of Excess Reactant Left Over

Starter Activity Balance the below equations: Mg + O2  MgO

Limiting reactant.

The Stoichiometry Game!

Mole Ratios Limiting Reagent Yield Gas Stoichiometry

Limiting Reactant.

Finding the Amount of Excess Reactant Left Over

Limiting reagents.

Stoichiometric Calculations

Reaction Yield.

% Yield Definitions 1. Theoretical Yield

Review #1 In the formation of carbon dioxide from carbon monoxide and oxygen, how many moles of carbon monoxide are needed to react completely with 7.0.

LIMITING REAGENT (LR) gets completely used up in the reaction

(STOY-KEE-AHM-EH-TREE)

Presentation transcript:

LIMITING REAGENT

LIMITING & EXCESS REACTANT Before the reaction has started After the reaction is complete CO (g) + 2 H 2 (g) CH 3 OH (g)

STEPS 1.Use stoichiometry to convert reactant(s) into the product 2.Identify limiting reactant (LR), excess reactant (ER), and max amount of product 3.To calculate how much in excess, subtract the max amount of product and use stoichiometry to convert back to grams of excess reactant

How many grams of silver bromide can be formed when solutions containing 50.0 g of magnesium bromide and g of silver nitrate are mixed together? What is the limiting reactant? What is in excess, and how much? MgBr 2 + AgNO 3 AgBr + Mg(NO 3 ) 2 EXAMPLE 1

How many grams of hydrogen chloride can be produced from 1.00 g of hydrogen and 55.0 g of chlorine? What is the limiting reactant? What is in excess, and how much? H 2 + Cl 2 HCl EXAMPLE 2

How many grams of barium sulfate will be formed from g of barium nitrate and g of sodium sulfate? What is the limiting reactant? What is in excess, and how much? Ba(NO 3 ) 2 + Na 2 SO 4 BaSO 4 + NaNO 3 EXAMPLE 3