STOICHIOMETRY What is stoichiometry l Stoichiometry is the
![STOICHIOMETRY STOICHIOMETRY](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-1.jpg)
![What is stoichiometry? l. Stoichiometry is the quantitative study of quantitative reactants and products What is stoichiometry? l. Stoichiometry is the quantitative study of quantitative reactants and products](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-2.jpg)
![Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction. Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction.](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-3.jpg)
![Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-4.jpg)
![Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-5.jpg)
![Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-6.jpg)
![Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-7.jpg)
![Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-8.jpg)
![D. P. S. E. l DECONSTRUCT- Identify what you 1) Know: Ratio (balanced equation) D. P. S. E. l DECONSTRUCT- Identify what you 1) Know: Ratio (balanced equation)](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-9.jpg)
![D. P. S. E. l Plan- Decide what type of pathway or equation you D. P. S. E. l Plan- Decide what type of pathway or equation you](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-10.jpg)
![D. P. S. E. l Solve – Insert numbers with units in proper places D. P. S. E. l Solve – Insert numbers with units in proper places](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-11.jpg)
![D. P. S. E. l Evaluate – Circle your answer with units, and check D. P. S. E. l Evaluate – Circle your answer with units, and check](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-12.jpg)
![What You Should Expect l l Given : Amount of reactants Question: how much What You Should Expect l l Given : Amount of reactants Question: how much](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-13.jpg)
![What do you need? i. iii. iv. You will need to use molar ratios, What do you need? i. iii. iv. You will need to use molar ratios,](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-14.jpg)
![Steps Involved in Solving Mass-Mass Stoichiometry Problems l l Balance the chemical equation correctly Steps Involved in Solving Mass-Mass Stoichiometry Problems l l Balance the chemical equation correctly](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-15.jpg)
![Mole Ratios A mole ratio converts moles of one compound in a balanced chemical Mole Ratios A mole ratio converts moles of one compound in a balanced chemical](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-16.jpg)
![Example Reaction between magnesium and oxygen to form magnesium oxide. (fireworks) 2 Mg(s) + Example Reaction between magnesium and oxygen to form magnesium oxide. (fireworks) 2 Mg(s) +](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-17.jpg)
![Practice Problems 1) N 2 + 3 H 2 ---> 2 NH 3 Write Practice Problems 1) N 2 + 3 H 2 ---> 2 NH 3 Write](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-18.jpg)
![Mole-Mole Problems Using the practice question 2) from the previous slide: Equation of reaction Mole-Mole Problems Using the practice question 2) from the previous slide: Equation of reaction](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-19.jpg)
![Mole to Mole Question (1) 4 NH 3 + 5 O 2 6 H Mole to Mole Question (1) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-20.jpg)
![Mole to Mole Question (2) 4 NH 3 + 5 O 2 6 H Mole to Mole Question (2) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-21.jpg)
![Mole-Mass Problems Make sure you have molar masses worked out for all compounds l Mole-Mass Problems Make sure you have molar masses worked out for all compounds l](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-22.jpg)
![Example for Mole-Mass Problems l Problem 1: 1. 50 mol of KCl. O 3 Example for Mole-Mass Problems l Problem 1: 1. 50 mol of KCl. O 3](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-23.jpg)
![Let’s go! Molar masses: 245. 10 1. 50 mol of KCl. O 3 decomposes. Let’s go! Molar masses: 245. 10 1. 50 mol of KCl. O 3 decomposes.](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-24.jpg)
![Try This: We want to produce 2. 75 mol of KCl. How many grams Try This: We want to produce 2. 75 mol of KCl. How many grams](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-25.jpg)
![Mole to Mass Question (3) 4 NH 3 + 5 O 2 6 H Mole to Mass Question (3) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-26.jpg)
![Mole to Mass Question (4) 4 NH 3 + 5 O 2 6 H Mole to Mass Question (4) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-27.jpg)
![Mass to Mass Question (5) 4 NH 3 + 5 O 2 6 H Mass to Mass Question (5) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-28.jpg)
![Have we learned it yet? Try these on your own - 4 NH 3 Have we learned it yet? Try these on your own - 4 NH 3](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-29.jpg)
- Slides: 29
![STOICHIOMETRY STOICHIOMETRY](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-1.jpg)
STOICHIOMETRY
![What is stoichiometry l Stoichiometry is the quantitative study of quantitative reactants and products What is stoichiometry? l. Stoichiometry is the quantitative study of quantitative reactants and products](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-2.jpg)
What is stoichiometry? l. Stoichiometry is the quantitative study of quantitative reactants and products in a chemical reaction. “stoichio” – Greek for element l “metry” = measurement l
![Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction.](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-3.jpg)
Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction. Consider the chemical equation: 4 NH 3 + 5 O 2 6 H 2 O + 4 NO There are several numbers involved. What do they all mean?
![Stoichiometry 4 NH 3 5 O 2 6 H 2 O 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-4.jpg)
Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 NO Recall that Chemical formulas represent numbers of atoms NH 3 1 nitrogen and 3 hydrogen atoms O 2 2 oxygen atoms H 2 O 2 hydrogen atoms and 1 oxygen atom NO 1 nitrogen atom and 1 oxygen atom
![Stoichiometry 4 NH 3 5 O 2 6 H 2 O 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-5.jpg)
Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 NO Recall that Chemical formulas have molar masses: NH 3 17 g/mol O 2 32 g/mol H 2 O 18 g/mol NO 30 g/mol ***To find the molar mass of a chemical formula – add the atomic masses of the elements forming the compound. Use the periodic table to determine the atomic mass of individual elements. ***
![Stoichiometry 4 NH 3 5 O 2 6 H 2 O 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-6.jpg)
Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 NO Recall that Chemical formulas are balanced with coefficients 4 X NH 3 = 4 nitrogen + 12 hydrogen 5 X O 2 = 10 oxygen 6 X H 2 O = 12 hydrogen + 6 oxygen 4 X NO = 4 nitrogen + 4 oxygen
![Stoichiometry 4 NH 3 5 O 2 6 H 2 O 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-7.jpg)
Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 NO With Stoichiometry we find out that 4 : 5 : 6 : 4 do more than just multiply atoms. 4 : 5 : 6 : 4 Are what we call a mole ratio.
![Stoichiometry 4 NH 3 5 O 2 6 H 2 O 4 Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-8.jpg)
Stoichiometry 4 NH 3 + 5 O 2 6 H 2 O + 4 NO 4 : 5 : 6 : 4 Can mean either: 4 molecules of NH 3 react with 5 molecules of O 2 to produce 6 molecules of H 2 O and 4 molecules of NO OR 4 moles of NH 3 react with 5 moles of O 2 to produce 6 moles of H 2 O and 4 moles of NO
![D P S E l DECONSTRUCT Identify what you 1 Know Ratio balanced equation D. P. S. E. l DECONSTRUCT- Identify what you 1) Know: Ratio (balanced equation)](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-9.jpg)
D. P. S. E. l DECONSTRUCT- Identify what you 1) Know: Ratio (balanced equation) 2) Know: from the problem 3) Need to find: from the problem
![D P S E l Plan Decide what type of pathway or equation you D. P. S. E. l Plan- Decide what type of pathway or equation you](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-10.jpg)
D. P. S. E. l Plan- Decide what type of pathway or equation you need to use. l We are going to start with using ratios, equalities, cross-multiplying and then dividing as needed (as we did last semester)
![D P S E l Solve Insert numbers with units in proper places D. P. S. E. l Solve – Insert numbers with units in proper places](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-11.jpg)
D. P. S. E. l Solve – Insert numbers with units in proper places in your Plan
![D P S E l Evaluate Circle your answer with units and check D. P. S. E. l Evaluate – Circle your answer with units, and check](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-12.jpg)
D. P. S. E. l Evaluate – Circle your answer with units, and check it to see if it makes sense. l Is it too big, too small, does it make logical sense?
![What You Should Expect l l Given Amount of reactants Question how much What You Should Expect l l Given : Amount of reactants Question: how much](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-13.jpg)
What You Should Expect l l Given : Amount of reactants Question: how much of the products can be formed. l Example l l 2 A + 2 B 3 C Given 20. 0 grams of A and sufficient B, how many grams of C can be produced?
![What do you need i iii iv You will need to use molar ratios What do you need? i. iii. iv. You will need to use molar ratios,](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-14.jpg)
What do you need? i. iii. iv. You will need to use molar ratios, molar masses, balancing and interpreting equations, and conversions between grams and moles.
![Steps Involved in Solving MassMass Stoichiometry Problems l l Balance the chemical equation correctly Steps Involved in Solving Mass-Mass Stoichiometry Problems l l Balance the chemical equation correctly](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-15.jpg)
Steps Involved in Solving Mass-Mass Stoichiometry Problems l l Balance the chemical equation correctly If mass is given: Using the molar mass of the given substance, convert the mass given to moles. Construct a molar proportion (two molar ratios set equal to each other) Using the molar mass of the unknown substance, convert the moles just calculated to mass.
![Mole Ratios A mole ratio converts moles of one compound in a balanced chemical Mole Ratios A mole ratio converts moles of one compound in a balanced chemical](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-16.jpg)
Mole Ratios A mole ratio converts moles of one compound in a balanced chemical equation into moles of another compound.
![Example Reaction between magnesium and oxygen to form magnesium oxide fireworks 2 Mgs Example Reaction between magnesium and oxygen to form magnesium oxide. (fireworks) 2 Mg(s) +](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-17.jpg)
Example Reaction between magnesium and oxygen to form magnesium oxide. (fireworks) 2 Mg(s) + Mole Ratios: 2 : O 2(g) 1 2 Mg. O(s) : 2
![Practice Problems 1 N 2 3 H 2 2 NH 3 Write Practice Problems 1) N 2 + 3 H 2 ---> 2 NH 3 Write](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-18.jpg)
Practice Problems 1) N 2 + 3 H 2 ---> 2 NH 3 Write the mole ratios for N 2 to H 2 and NH 3 to H 2. 2) A can of butane lighter fluid contains 1. 20 moles of butane (C 4 H 10). Calculate the number of moles of carbon dioxide given off when this butane is burned.
![MoleMole Problems Using the practice question 2 from the previous slide Equation of reaction Mole-Mole Problems Using the practice question 2) from the previous slide: Equation of reaction](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-19.jpg)
Mole-Mole Problems Using the practice question 2) from the previous slide: Equation of reaction 2 C 4 H 10 + 13 O 2 8 CO 2 + 10 H 2 O Mole ratio C 4 H 10 CO 2 Know from bal eq: 2 : 8 [ coefficients] Simplify if needed: 1 : 4 What to Find: 1. 2 : X [ problem] By cross-multiplication: (4)(1. 2) = (1)(x) X = 4. 8 mols of CO 2 given off
![Mole to Mole Question 1 4 NH 3 5 O 2 6 H Mole to Mole Question (1) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-20.jpg)
Mole to Mole Question (1) 4 NH 3 + 5 O 2 6 H 2 O + 4 NO l How many moles of H 2 O are produced if 2. 00 moles of O 2 are used? Notice that a correctly balanced equation is essential to get the right answer
![Mole to Mole Question 2 4 NH 3 5 O 2 6 H Mole to Mole Question (2) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-21.jpg)
Mole to Mole Question (2) 4 NH 3 + 5 O 2 6 H 2 O + 4 NO How many moles of NO are produced in the reaction if 15 mol of H 2 O are also produced?
![MoleMass Problems Make sure you have molar masses worked out for all compounds l Mole-Mass Problems Make sure you have molar masses worked out for all compounds l](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-22.jpg)
Mole-Mass Problems Make sure you have molar masses worked out for all compounds l Set up for grid making sure to use units correctly l Cross-multiply and isolate your variable (be sure to recognize those units that cancel out) l
![Example for MoleMass Problems l Problem 1 1 50 mol of KCl O 3 Example for Mole-Mass Problems l Problem 1: 1. 50 mol of KCl. O 3](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-23.jpg)
Example for Mole-Mass Problems l Problem 1: 1. 50 mol of KCl. O 3 decomposes. How many grams of O 2 will be produced? [K = 39, Cl = 35. 5, O = 16] 2 KCl. O 3 2 KCl + 3 O 2
![Lets go Molar masses 245 10 1 50 mol of KCl O 3 decomposes Let’s go! Molar masses: 245. 10 1. 50 mol of KCl. O 3 decomposes.](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-24.jpg)
Let’s go! Molar masses: 245. 10 1. 50 mol of KCl. O 3 decomposes. How many grams of O 2 will be produced? 149. 10 96 2 KCl. O 3 2 KCl + 3 O 2 2 mol : 96 g 1. 50 mol : X g (96 g)(1. 50 mol)=(2 mol)(X g) 144 g/mol = (2 mol) (X g) 144 g/mol / 2 mol = 72 g O 2
![Try This We want to produce 2 75 mol of KCl How many grams Try This: We want to produce 2. 75 mol of KCl. How many grams](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-25.jpg)
Try This: We want to produce 2. 75 mol of KCl. How many grams of KCl. O 3 would be required? Soln l KCl. O 3 KCl : 245. 10 g : 2 mol X g : 2. 75 mol (2 mol)(X g) = (2. 75 mol)(245. 10 g) (2 mol)(X g) = 674. 025 g/mol X = 337. 01 grams of KCl. O 3
![Mole to Mass Question 3 4 NH 3 5 O 2 6 H Mole to Mass Question (3) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-26.jpg)
Mole to Mass Question (3) 4 NH 3 + 5 O 2 6 H 2 O + 4 NO l How many grams of H 2 O are produced if 2. 2 mol of NH 3 are combined with excess oxygen?
![Mole to Mass Question 4 4 NH 3 5 O 2 6 H Mole to Mass Question (4) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-27.jpg)
Mole to Mass Question (4) 4 NH 3 + 5 O 2 6 H 2 O + 4 NO l How many grams of O 2 are required to produce 0. 3 mol of H 2 O?
![Mass to Mass Question 5 4 NH 3 5 O 2 6 H Mass to Mass Question (5) 4 NH 3 + 5 O 2 6 H](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-28.jpg)
Mass to Mass Question (5) 4 NH 3 + 5 O 2 6 H 2 O + 4 NO l How many grams of NO is produced if 12 g of O 2 is combined with excess ammonia?
![Have we learned it yet Try these on your own 4 NH 3 Have we learned it yet? Try these on your own - 4 NH 3](https://slidetodoc.com/presentation_image_h/28356fa66c14ba75942916a802705e22/image-29.jpg)
Have we learned it yet? Try these on your own - 4 NH 3 + 5 O 2 6 H 2 O + 4 NO a) How many moles of H 2 O can be made using 1. 6 mol NH 3? b) What mass of NH 3 is needed to make 0. 75 mol NO? c) How many grams of NO can be made from 47 g of NH 3?
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