Review: Mole Conversions: Convert 3 mols Oxygen to grams: Convert 42 grams Chlorine to mols: What is % composition? What is the %comp of magnesium in magnesium.

Slides:



Advertisements
Similar presentations
STOICHIOMETRY.
Advertisements

Stoichiometry (Yay!).
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.
CH 10: Chemical Equations & Calcs
Mathematics of Chemical Equations By using “mole to mole” conversions and balanced equations, we can calculate the exact amounts of substances that will.
Ch. 9 Notes – Chemical Quantities
WHAT DO THE COEFFICIENTS IN A REACTION TELL US??!?!
Stoichiometry.
Starter S moles NaC 2 H 3 O 2 are used in a reaction. How many grams is that?
Ch. 9 Notes -- Stoichiometry
Section 3.7 Limiting Reactants Grilled Cheese Sandwich Bread + Cheese  ‘Cheese Melt’ 2 B + C  B 2 C 100 bread 30 slices ? sandwiches What is the limiting.
Chapter 9 Stoichiometry
Limiting Reagent and Percent Yield
“Stoichiometry” Original slides by Stephen L. Cotton Mr. Mole.
Classic Butter Cookies 2 1/2 cups all-purpose flour 1 cup butter 1/2 cup white sugar 2 eggs 1/2 teaspoon almond extract Bake at 350ºF for 10 minutes.
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.
April 3, 2014 Stoichiometry. Stoichiometry is the study of quantities of materials consumed and produced in chemical reactions Stoikheion (Greek, “element”)
Stoichiometry Chapter 8. Stoichiometry Chemical equations Limiting reagent Problem types Percent yield Mass-mass Mole - mole other.
Chapter 12: Stoichiometry
Stoichiometry Chapter 9.
Stoichiometry. Information Given by the Chemical Equation  The coefficients in the balanced chemical equation show the molecules and mole ratio of the.
Starter S moles of Iron (III) Hydroxide are used in a reaction. How many grams is that?
Stoichiometry Chapter 9 Limiting reagents. In Stoichiometry: We work in moles. We cannot calculate grams of product from grams of reactant.
Limiting Factors & Percent Yield Quiz. Bell Ringer When 6.58 g SO 3 and 1.64 g H 2 O react, what is the expected yield of sulfuric acid? If the actual.
STOICHIOMETRY Chapter 9 Stoichiometry Mole-Mole Mass-Mole Mass-Mass
The Mole & Stoichiometry!
Ch. 9 Notes – Chemical Quantities
Gravimetric Stoichiometry Is used to calculate masses of reactants and products in a reaction.
Chapter 12: Stoichiometry 12.1 The Arithmetic of Equations.
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.
It’s time to learn about.... Stoichiometry Stoichiometry : Mole Ratios to Determining Grams of Product At the conclusion of our time together, you should.
Ch. 9 Notes – Chemical Quantities Stoichiometry refers to the calculations of chemical quantities from __________________ chemical equations. Interpreting.
Chapter 9 “Stoichiometry” Chemistry Charles Page High School Stephen L. Cotton.
Stoichiometry and cooking with chemicals.  Interpret a balanced equation in terms of moles, mass, and volume of gases.  Solve mole-mole problems given.
Video 9-1 Reaction Stoichiometry Steps for Problem Solving.
Ch. 9 Notes -- Stoichiometry Stoichiometry refers to the calculations of chemical quantities from __________________ chemical equations. Interpreting Everyday.
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)
When gases react, the coefficients in the balanced chemical equation represent both molar amounts and relative volumes. Section 3: Gas Stoichiometry K.
Stoichiometry. What is stoichiometry? Involves the mass relationships between reactants and products in a chemical reaction ▫Based on the law of conservation.
Stoichiometry GPS 13. 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 mol H 2 O 1 mol O.
TOPIC 17: INTRO TO STOICHIOMETRY EQ: EQ: How does a balanced chemical equation help you predict the number of moles and masses of reactants and products?
Chemistry Chapter 9 - Stoichiometry South Lake High School Ms. Sanders.
Chapter 9 + review. Chapter 9: Chemical quantities Information given by chemical equations –Chem. eq. tell us amt. of reactant(s) needed to get to the.
SOL Review 6 Stoichiometry. Consider: 4NH 3 + 5O 2  6H 2 O + 4NO Many conversion factors exist: 4 NH 3 6 H 2 04NO 5O 2 (and others) 5 O 2 4 NO4 NH 3.
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.
Stoichiometry – Ch What would be produced if two pieces of bread and a slice of salami reacted together? + ?
Stoichiometry Chapter 12. 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.
Stoichiometry Chemistry I: Chapter 12 Chemistry I HD: Chapter 9 SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead.
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.
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.
Let’s talk… mole to mole
Stoichiometry The calculation of quantities in chemical equations.
Intro to Ch 9 Pg 267 #2= work w/partner (a-f)=10 min
Stoichiometry II.
Ch. 9 Notes -- Stoichiometry
Stoichiometry.
Stoichiometry Unit 7.
Stoichiometry.
MASS - MASS STOICHIOMETRY
Equation Calculations
Ch. 8 Stoichiometry.
Chemical Reactions Unit
Limiting Reactant/Reagent Problems
Mathematics of Chemical Equations
Stoichiometry Unit 4 (Ch 9).
Ch. 9 Notes -- Stoichiometry
Chemical Calculations
Stoichiometry.
Presentation transcript:

Review: Mole Conversions: Convert 3 mols Oxygen to grams: Convert 42 grams Chlorine to mols: What is % composition? What is the %comp of magnesium in magnesium nitrate?

Stoichiometry Stoichiometry refers to the calculations of chemical quantities from balanced chemical equations. Where do we use this? Stoichiometry is used to determine the amount of reactant or product necessary to complete a reaction. Why is it important? This can be used in factories to make sure the appropriate amount of product is made with the least amount of waste.

Practical problems Let’s first look at stoichiometry in our lives. What makes up a grilled cheese? ___Bread slices + ___Cheese ___ Grilled Cheese How many slices of bread are needed to make 24 Grilled cheese sandwiches? How many grilled cheese can be made with 12 slices of cheese? Butter

Interpreting Chemical Equations The first thing that must be done is to balance the equation! N2 (g) + H2 (g)  NH3 (g) Here are the kinds of information you can get from the equation: ____ mole N2 + ____ moles H2  ____ moles NH3 ___ molecule N2 + ___ molecules H2  ___ molecules NH3 ____ liter N2 + ____ liters H2  ____ liters NH3 ____ grams N2 + ____ grams H2  ____ grams NH3

Mole-Mole Conversions When we are given an amount of moles in a reaction, we can find the amounts of the other reactants/products. A mole ratio is needed to convert from one mole to another. We find the mole ratio in the balanced equation. The mole conversion factor comes from the coefficients of the balanced chemical equation. Step 1: Write down the what you know. Step 2: Use a mole ratio to convert.

Practice Problems: N2 (g) + 3H2 (g)  2NH3 (g) 1) How many moles of ammonia can be made from 7 moles of nitrogen reacting with an excess of hydrogen? 2) How many moles of hydrogen are required to completely react with 8 moles of nitrogen to produce ammonia? 3) How many moles of hydrogen are needed to react with an excess of nitrogen to make 10 moles of ammonia?

What If you are given MASS??? Mass-Mass: (grams  moles  moles  grams) Step 1: Write down what you know. Step 2: Use Molar mass to convert to mols. Step 3: Use a mole ratio from your balanced equation. Step 4: Use molar mass to convert to grams. N2 (g) + 3H2 (g)  2NH3 (g) Practice Problem: How many grams of ammonia can be made from reacting 39.0 grams of nitrogen with an excess of hydrogen?

Other Conversion Problems Volume-Mass: (liters  moles  moles  grams) Step 1: Write down what you know. Step 2: Use (1 mol @STP = 22.4 L) to convert to mols. Step 3: Use a mole ratio from your balanced equation. Step 4: Use molar mass to convert to grams. N2 (g) + 3H2 (g)  2NH3 (g) Practice Problem: How many grams of ammonia can be made from reacting 20.0 liters of hydrogen with an excess of nitrogen?

Other Conversion Problems Mass-Volume: (grams to moles to moles to liters) Step 1: Write down what you know. Step 2: Use molar mass to convert to mols. Step 3: Use a mole ratio from your balanced equation. Step 4: Use (1 mol @STP = 22.4 L) to convert to Liters. N2 (g) + 3H2 (g)  2NH3 (g) Practice Problem: How many liters of ammonia can be made from reacting 36.0 grams of nitrogen with an excess of hydrogen?

Other Conversion Problems Volume-Volume: (exactly like mole-mole) Step 1: Write down the what you know. Step 2: Use a mole (But with Liters as units) fraction to convert. N2 (g) + 3H2 (g)  2NH3 (g) Practice Problem: How many liters of ammonia can be made from reacting 125 liters of hydrogen with an excess of nitrogen?

Percent Yield The Percent Yield is a ratio that tells us how efficient a chemical reaction is. - The higher the % yield, the more efficient the reaction is. (Unless you go over 100%) Actual Yield Theoretical Yield The actual yield is the amount you experimentally produce when you run the reaction in a lab. The theoretical yield is the amount you are ideally produce if everything goes perfectly. You can calculate this amount using stoichiometry! % Yield = x 100

How to Calculate Percent Yield Step 1: Calculate the theoretical yield for the problem. (This means doing the stoichiometry for the problem) Step 2: Divide the actual yield by the theoretical yield. Step 3: Multiply by 100

Practice Problem: 2H2 (g) + O2 (g)  2H2O (g) 1) A student reacts 40 grams of hydrogen with an excess of oxygen and produces 300 grams of water. Find the % yield for this reaction.

Practice Problem: 2H2 (g) + O2 (g)  2H2O (g) 2) If 2.0 grams of hydrogen completely reacted with 16.0 grams of oxygen but only produced 17.5 grams of water, what is the % yield for the reaction?

FOR THE FIRST 5 MINUTES! Get into your lab groups from last week. Work TOGETHER on the following Problem a. Write the equation for the reaction of iron (III) phosphate with sodium sulfate to produce iron (III) sulfate and sodium phosphate.    b. If I perform this reaction with 25 grams of iron (III) phosphate and an excess of sodium sulfate, how many grams of iron (III) sulfate can I make?    c. If 18.5 grams of iron (III) sulfate are actually made, what is my percent yield? Sulfate: SO4-2 Phosphate: PO4-3

Limiting Reactant The limiting reactants is the reactant that runs out first. It “limits” the reaction from continuing (when it is used up). The reactant that is in abundance is called the excess reactant.

How to find the Limiting Reactant Step 1: If given grams, convert reactants to Mols of a product. Step 2: Compare the amount of product. The reactant that makes less product is the limiting reactant. If I give you a quantity for both reactants, you must find the limiting reactant before finding the final amount of product. If I say THE HYDROGEN IS USED COMPLETELY… What does this mean?

Practice Problems:___N2 (g) +___H2 (g)  ___NH3 (g) 1) If 2 Practice Problems:___N2 (g) +___H2 (g)  ___NH3 (g) 1) If 2.7 moles of nitrogen reacts with 6.3 moles of hydrogen, which will you run out of first? 2) If 3.9 moles of nitrogen reacts with 12.1 moles of hydrogen, what is the limiting reagent?

How to calculate Excess Reactant How many moles of excess reagent do you have? PRE-STEP 1: You must know which reactant is in excess! Step 1: Start with the amount of product will be produced from the limiting reactant. Step 2: Convert this to mols of the reactant in excess. Step 3: Subtract this amount from the original amount.

Practice Problem: N2 + 3H2  2NH3 1) If 2.7 moles of nitrogen reacts with 6.3 moles of hydrogen, how much excess reactant will you have? 2) If 3.9 moles of nitrogen reacts with 12.1 moles of hydrogen, how much excess reactant will you have?