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,

Slides:

Advertisements

Similar presentations

Chapter 9 - Section 3 Suggested Reading: Pages

Advertisements

Chapter 12 Stoichiometry.

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.

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

Mass relationships in chemical reactions: Stoichiometry

Chapter 9 Stoichiometry.

CHEMISTRY February 13, 2012.

Stoichiometry Chemistry Ms. Piela.

AP Chemistry Chap. 3 Stoichiometry, Part Chemical Equations (p. 100)- shows a chemical change. Reactants on the LHS, products on the RHS. Bonds.

Percent Yield and Limiting Reactants

Limiting Reactant.  Determine which reactant is left over in a reaction.  Identify the limiting reactant and calculate the mass of the product.  Calculate.

Limiting Reactant.

How many moles of water will be produced when 8 grams of hydrogen gas react with the oxygen in the air? Episode 801.

Starter S moles NaC 2 H 3 O 2 are used in a reaction. How many grams is that?

STOICHIOMETRY.  Stoichiometry is the science of using balanced chemical equations to determine exact amounts of chemicals needed or produced in a chemical.

STOICHIOMETRY CALCULATIONS COACH COX. MOLE TO MOLE CONVERSIONS Converting from moles of one substance in a chemical reaction to moles of another substance.

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

Stoichiometry The Math of Chemical Reactions Unit 9.

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.

Stoichiopardy Holy Moley Do the 2 or 3 step Random Limit my Percent Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400 Q $500 Final Chempardy.

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

Stoichiometry II. Solve stoichiometric problems involving moles, mass, and volume, given a balanced chemical reaction. Include: heat of reaction Additional.

Percent Yield Section 12.4.

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.

Chapter 12 Review “Stoichiometry”

Stoichiometry Calculations based on Chemical Reactions.

Test Review Chemical Reactions and Stoichiometry.

The Mole Stoichiometry Limiting Reactant % Yield

Limiting Reactants and Percent Yield

Stoichiometry. What Is It? Branch of chemistry that shows the relationships among reactants and products in a chemical reaction Equations must be balanced.

The Mathematics of Chemical Reactions Chemical Stoichiometry Quantitative Relationships between the reactants and products in a chemical reaction.

Relative Formula Mass expressed in grams

The Mole & Stoichiometry!

II. Stoichiometry in the Real World Stoichiometry.

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

Chap. 9: Stoichiometry Identify the mole ratio of any two species in a chemical reaction. Calculate theoretical yields from chemical equations.

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

The Math of Chemical Reactions

What is stoichiometry? A problem solving method used to calculate the amount of product made or amount of reactant needed in a chemical reaction What is.

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.

Honors Stoichiometry Examples. Example 1 What mass of carbon dioxide in grams is needed to react with 3.00mol of H 2 O in the following photosynthetic.

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,

 How far away you are from a theoretical or “actual” value.

% 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.

Limiting Reactants, Theoretical Yield, and % Yield.

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.

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 ?

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

Mass-Mass Conversions 56.0 g N 2 x g N 2 g NH = 1904 = When nitrogen and hydrogen react, they form ammonia gas, which has the formula.

Honors Stoichiometry Examples. Example 1 What mass of carbon dioxide in grams is needed to react with 3.00mol of H 2 O in the following photosynthetic.

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

Stoichiometry II.

Stoichiometry Stoichiometry: is the study of the calculations of amounts of substances involved in chemical equations.

Finding the Amount of Excess Reactant Left Over

II. Stoichiometry in the Real World

Chapter 12 Review.

Chapter 12 Review.

Finding the Amount of Excess Reactant Left Over

Stoichiometry Review.

How many moles of water are made by

STOICHIOMETRY REVIEW.

Stoichiometry Unit 7 Lesson 1.

Yield-noun: Performance, production, product. Harvest, crop.

Presentation transcript:

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, how many grams of ammonia will be produced? Episode 802 N 2 (g) + 3H 2 (g)  2NH 3 (g) ? g NH 3 = 56.0 g N 2 28g N 2 1 mol N 2 1 mol NH 3 2 mol NH 3 17g NH 3 = 68g NH 3

Sodium metal reacts with oxygen to produce solid sodium oxide. How many grams of sodium must react to produce 42.0 grams of sodium oxide? When 12.0 grams of hydrogen reacts with oxygen, how many grams of water are produced? 4Na (s) + O 2 (g)  2Na 2 O (s) 2H 2 (g) + O 2 (g)  2H 2 O (l) ? g Na = 42.0g Na 2 O 62g Na 2 O 1 mol Na 2 O 2 mol Na 2 O 4 mol Na 1 mol Na 23g Na = 31g Na ? g H 2 O = 12.0g H 2 2g H 2 1 mol H 2 2 mol H 2 2 mol H 2 O 1 mol H 2 O 18g H 2 O = 108g H 2 O Episode 802

Actual Yield – Amount of product produced when the reaction is performed in a lab Theoretical Yield – Amount of product expected to be produced based on the balanced equation and the amount of reactants – Calculated using stoichiometry Percent Yield – (actual yield/theoretical yield) x 100% Episode 802

Percent Yield in Lab Actual yield of CO 2 = 0.13g – (from lab data) Calculated theoretical yield from the balanced equation: NaHCO 3 + HCl  NaCl + CO 2 + H 2 O ? g CO 2 = 0.23g NaCO 3 84g NaCO 3 1mol NaCO 3 1mol CO 2 44g CO 2 = 0.12g CO 2 % yield = 0.13g 0.12g x 100 = 108% Episode 802

What is the % yield of carbon dioxide when 5.99 grams of propane are burned and grams of carbon dioxide are collected? C 3 H 8 + 5O 2  3CO 2 + 4H 2 O ? g CO 2 = 5.99g C 3 H 8 44g C 3 H 8 1 mol C 3 H 8 3 mol CO 2 1 mol CO 2 44g CO 2 = 17.97g CO 2 % yield = g 17.97g x 100 = 67% Episode 802