Limiting Reagents Determine the mass of P 4 O 10 formed if 25g P 4 and 50g O 2 are combined. P 4 + 5O 2  P 4 O 10 What is the given? We have to find the.

Slides:

Advertisements

Similar presentations

Performing Calculations involving Limiting and Excess Reagents.

Advertisements

(Stoo-eek-ee-aam-et-ry)

Stoichiometric Calculations

Limiting Reactants and Percent Yield

Chapter 12 Notes #3 Limiting and Excess

Limiting Reactants.

Limiting Reactants & Percent Yield. Limiting Reactants  The reactant that limits the amount of product formed in a chemical reaction. The quantity of.

Laboratory 08 LIMITING REACTANT LAB.

Chapter 9 Chemical Quantities. 9 | 2 Information Given by the Chemical Equation Balanced equations show the relationship between the relative numbers.

Chemistry Week 26 Please get out your calculator!.

Limiting Reactants and Percent Yields

Limiting Reactants and Excess

Limiting Reactants & Percent Yield

Limiting Reagents Excess Reagents Percent yield

Limiting Reagent and Percent Yield

Limiting Reagents and Percent Yield

Identify the limiting reactant and calculate the mass of a product, given the reaction equation and reactant data. Include: theoretical yield, experimental.

Is this a balanced eq ? We only need ONE information during the reaction (reacted or produced)

Chapter 9 – STOICHIOMETRY

Chapter 12 Stoichiometry Anything in black letters = write it in your notes (‘knowts’) 12.1 – The Arithmetic of Equations 12.2 – Chemical Calculations.

Percentage Yield.

11-3 Limiting Reactants Reactions to this point have had one ingredient in excess. When you are given two or both reactant amounts, you have a limiting.

4.3 Limiting Reactant, Theoretical Yield and Percent Yield.

Chapter 10 Stoichiometry Or One plus One isn’t always Two.

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 ?

Limiting Reagents and Percent Yield Using Stoichiometry.

Chapter 9 – STOICHIOMETRY The MATH of a CHEMICAL REACTION.

Chapter 12 Stoichiometry. 1. The part of chemistry that deals with the amount of substances involved in chemical reactions A. 3 basic steps to every stoichiometry.

Theoretical yield vs. Actual yield. Suppose the theoretical yield for an experiment was calculated to be 19.5 grams, and the experiment was performed,

Theoretical yield: amounts of product calculated from the limiting reagent. Actual yield: amount produced during the conducted experiment. Percentage.

PERCENT YIELD. Percent Yield Percent yield is the ratio of actual yield of an experiment to theoretical yield. To find percent yield, you divide the actual.

Limiting Reagent and Percent Yield Chapter 12.3 Page 368.

Chapter 9 - Stoichiometry

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

Theoretical Yield and Percent Yield Recipe says makes 3 dozen, you get 30. Your percent yield is 83.33%.

Percentage Yield.

It’s time to learn about... Stoichiometry: Limiting Reagents At the conclusion of our time together, you should be able to: 1. Determine the limiting.

GOOD AFTERNOON! Prepare to take notes. You will be allowed to use these notes on the test next week! You will need: 1.Something to write on 2.Something.

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

WARM UP The reaction of iron ore with carbon follows the equation: 2 Fe 2 O C  4 Fe + 3 CO 2. How many moles of Fe can be produced from 37 moles.

LIMITING REACTIONS INB PAGE 43. ESSENTIAL QUESTION: Why is the limiting reactant not always the reactant with fewer moles?

Stoichiometry From the Greek words “stoicheion” meaning “element”

Chapter 12 Stoichiometry

Stoichiometry Limiting reagents

Combustion Analysis A g sample composed of C, H, N is burned to produce g CO2 and g H2O Assume all C in the sample is converted to CO2.

Limiting Reactants and Percent Yield

UNIT 11 STOICHIOMETRY Stoichiometry is the study of quantitative relationships between the amounts of reactants used and amounts of products formed by.

Finding the Amount of Excess Reactant Left Over

Chemistry I Objectives Chapter 11

Chapter 10 Stoichiometry

Warm -Up What is the name of the compound

Combustion Analysis A g sample composed of C, H, N is burned to produce g CO2 and g H2O Assume all C in the sample is converted to CO2.

Limiting Reactants.

Limiting Reactants.

WARM UP 4 Li + O2  2 Li2O If you have 804 g of Li available for the reaction, calculate the amount of O2 you will need to pump into the reaction to ensure.

Finding the Amount of Excess Reactant Left Over

Stoichiometry Comes from the Greek words stoicheion, meaning “element,” and metron, meaning “measure.”

Stoichiometry Vocab Theoretical Yield: the calculated amount of product yielded by a reaction (found through stoichiometry) Actual Yield: the actual amount.

Limiting Reactants.

Results Data Mass of iron nails before the reaction _________

Stoichiometry Chapter 12.

Stoichiometry & Limiting Reactants

Limiting Reactants and Percent Yield

Limiting Reactants and Percent Yield

Limiting Reagents Problem: Find the amount of cakes we can make when we have 4 sticks of butter and 50 cups of flour. 1 Butter + 2 Flour -> 1 Cake We.

Limiting Reactants and Percent Yield

#5 of 11-6 LIMITING REAGENT SET

Limiting Reactants.

Presentation transcript:

Limiting Reagents Determine the mass of P 4 O 10 formed if 25g P 4 and 50g O 2 are combined. P 4 + 5O 2  P 4 O 10 What is the given? We have to find the limiting reagent! 1 Mole P 4 5 Mole O 2 32 g O 2 25 g P 4 X X X = g O g P 4 1 Mole P 4 1 Mole O 2

Limiting Reagent O 2 was what we got when we used up all of our P 4. We have to now compare how much we used, to how much we had. We had 50 g O 2. We used g O 2. We therefore had g O 2 left over, in other words, in excess. Since we have O 2 left over, but have used up all of our P 4, we now know that O 2 is our excess reagent. This means that P 4 is our limiting reagent.

Limiting Reagent We now know to use P4, our limiting reagent as our given. This is because we can only produce as much product as our limiting reagent will allow. Think of it this way: We have 5 bicycle frames, and 20 wheels, how many bicycles can we produce? Frames: 5 bikes Wheels: 10 bikes We can only make 5 bikes, because frames are our limiting reagent!

Limiting Reagents Determine the mass of P 4 O 10 formed if 25g P 4 and 50g O 2 are combined. P 4 + 5O 2  P 4 O 10 The limiting reagent was P4, therefore we use P4 as our given to solve. 1 Mole P 4 1 Mole P 4 O g P 4 O g P 4 X X X = g P 4 O g P 4 1 Mole P 4 1 Mole P 4 O 10

Percent Yield Calculations If 100 g of Na and 100 g of Fe 2 O 3 are used in this reaction, how much Na 2 O, can be made? 6Na + Fe 2 O 3  Na 2 O + 2Fe 1 Mole Na 1 Mole Fe 2 O g Fe 2 O g Na X X X = g Fe 2 O 3 23 g Na 6 Mole Na 1 Mole Fe 2 O 3 Fe 2 O 3 is limiting

Percent Yield Calculations If 100 g of Na and 100 g of Fe 2 O 3 are used in this reaction, how much Na 2 O, can be made? 6Na + Fe 2 O 3  Na 2 O + 2Fe 1 Mole Fe 2 O 3 1 Mole Na 2 O 62 g Na 2 O 100 g Fe 2 O 3 X X X = g Na 2 O 160 g Fe 2 O 3 1 Mole Fe 2 O 3 1 Mole Na 2 O This is the theoretical yield!

Percent Yield Calculations Calculate the percent yield if the reaction actually yields 28.6 g of Na 2 O g Na2O was our theoretical. It is our theoretical because we had to do the math on paper. Actual 28.6 Theoretical X 100 =X 100 = 73.81%