The Basics of Stoichiometry and Mole Calculations References

The Basics of Stoichiometry and Mole Calculations References and Resources • Our TB: Ch. 3 of Chemistry: The central Science AP version (10 th edition) • Powerpoint *and in-class work • POGIL activities • Online resources for our TB (in particular: Practice Quiz and e-book) • Concept map for Stoichiometry and problem solving (handout) • Video lectures from chem guy (see next page) • Chem tours from ch. 3 of the W. W. Norton online book by Gilbert: • http: //www. wwnorton. com/college/chemistry/gilbert 2/contents/ch 03/studyplan. asp • *Some figures and examples in this PPT file have been taken from Melissa Brophy’s presentation at http: //teacherweb. com/TX/Mc. Neil. HS/brophy/photo 2. aspx

Resources: Video lectures for Chemistry • Chemguy videos (google AP chemistry and chemguy videos; use in sequence) (good, short, video lectures that are appropriate for regular, honors, or AP chemistry) • chem Guy video for mole 1 http: //www. youtube. com/watch? v=xi. Vwe. Bpj. XJo&playnext=1&videos=k. Hh 8 a 0 f. ILu. Y&feature=mfu_ in_order Mole 2 chem guy: http: //www. youtube. com/watch? v=xqw 2 BWd. Kl 1 Q&feature=Play. List&p=C 09489 B 20 AE 215 DF&pla ynext=1&playnext_from=PL&index=19 Mole 3 (Junior) : http: //www. youtube. com/watch? v=O 7 qj. YRYxkso&feature=Play. List&p=C 09489 B 20 AE 215 DF&playn ext=1&playnext_from=PL&index=20 • • • Stoichiometry video with worked example for predicting amount of product from 2. 6 mol of one of reactant: see http: //www. youtube. com/watch? v=-W 9 -s. Nf. M 5 Xo&feature=related Empirical formula for AP chem with chem. Guy: http: //www. youtube. com/watch? v=f. FXt. X_8 Ngs. Q&feature=related

The Basics of Stoichiometry and Mole Calculations Topics (review and new) • Reading and writing chemical equations • Balancing Equations • Types of reactions • Formula Weights and Molar Masses • Percent composition • Avagadro’s Number (continued) • Mole calculations • Solving problems using dimensional analysis using (1) Avagadro’s number, (2) GFM, or (3) mole ratios from coefficients of balanced equations • Determining Empirical formulas and Molecular formulas • Limiting reagents(reactants)

Chemical Equations • Symbolic representations or descriptions of chemical reactions • Meaning of the symbols, subscripts, parenthesis, + signs, arrows, co-efficients, states of matter, etc. Vocab. terms: reactants, products, catalyst, reaction conditions , etc. • Use of particle diagrams (to represent) • Conservation of Mass • Resources: POGIL activity “Chemical Reaction Equations” (To Do)

Reading Balanced Chemical Equations Molecules Particle diagrams Mass (amu) Amount (mol) Mass (g)

Balancing Equations Objective: find the smallest whole number ratio of coefficients for reactants and products that respects the law of conservation of mass. How? • Trial and error to some extent • Can Not change subscripts in chemical formulas but you Can change co-efficients in front of the formulas • Start by balancing those elements that occur in the fewest chemical formulas • Move back and forth checking the atom count each time a co-efficient is changed

Practice Balancing Equations • (example of a decomposition reaction that is used in air bags in cars)

Practice Balancing Equations (Index card activity – to hand in) • (example of a combustion reaction) • (Hint: Start with the element that occurs in the fewest chemical formulas)

Formula Weights • Atomic masses of atoms, molecules and formula unit • Atoms: • Ex: Au (gold) • One atom of Au has a mass of _____amu • Calculating formula weights in amu using chemical formula and the atomic masses from the periodic table • Ex: Na. Cl • One formula unit of Na. Cl has a mass of ______amu • Ex: C 6 H 12 O 6 (glucose) • One molecule of glucose has a mass of ______amu

Percent Composition What is the percent carbon in C 5 H 8 NO 4 (the glutamic acid used to make MSG monosodium glutamate), a compound used to flavor foods and tenderize meats?

Percent Composition What is the percent carbon in C 5 H 8 NO 4? Step 1: First calculate the Formula weight for the compound (FW for C 5 H 8 NO 4 is ____amu) Step 2: % composition = (mass of part ÷mass of whole) X 100 or % element = (# atoms of that element)(atomic weight of the element) x 100 Formula weight of the compound

What is the % carbon in MSG? Step 1: FW for C 5 H 8 NO 4 is ____amu C H N O

% Composition of Carbon in C 5 H 8 NO 4 Step 2 % C = (mass of part ÷mass of whole) X 100 or % element = (# atoms of element)(atomic weight of the element) x 100 Formula weight of the compound Answer?

Percent Composition What is the percent carbon in C 5 H 8 NO 4 (the glutamic acid used to make MSG monosodium glutamate), a compound used to flavor foods and tenderize meats? a) 8. 22 %C b) 24. 3 %C c) 41. 1 %C

Avagadro’s number and The Mole 6. 02 x 23 10 602, 000, 000, 000

The Mole • A counting unit • Similar to a dozen, except instead of 12, it’s 602 billion trillion 602, 000, 000, 000 • 6. 02 X 1023 (in scientific notation) • This number is named in honor of Amedeo _____ (1776 – 1856), 1856) who studied quantities of gases and discovered that no matter what the gas was, there were the same number of molecules present

How big of a unit is a mole? • If you had Avogadro's number of unpopped popcorn kernels, and spread them across the United States of America, the country would be covered in popcorn to a depth of over 9 miles.

The Mole (abbreviated as mol) • 1 dozen cookies = 12 cookies • 1 mole of cookies = 6. 02 X 1023 cookies • 1 dozen cars = 12 cars • 1 mole of cars = 6. 02 X 1023 cars • 1 dozen Al atoms = 12 Al atoms • 1 mole of Al atoms = 6. 02 X 1023 atoms Note that the NUMBER is always the same, but the MASS is very different!

A Mole of Particles Contains 6. 02 x 1023 particles 1 mole C = 6. 02 x 1023 C atoms 1 mole H 2 O = 6. 02 x 1023 H 2 O molecules 1 mole Na. Cl = 6. 02 x 1023 Na. Cl “formula units” (technically, ionic compounds are not molecules so they are called formula units) 6. 02 x 1023 Na+ ions and 6. 02 x 1023 Cl– ions

Avogadro’s Number as Conversion Factor 6. 02 x 1023 particles 1 mole or 1 mole 6. 02 x 1023 particles Note that a particle could be an atom OR a molecule!

Learning Check 1. Number of atoms in 0. 500 mole of Al a) 500 Al atoms b) 6. 02 x 1023 Al atoms c) 3. 01 x 1023 Al atoms 2. Number of moles of S in 1. 8 x 1024 S atoms a) 1. 0 mole S atoms b) 3. 0 mole S atoms c) 1. 1 x 1048 mole S atoms

Practice Problems – with /without using your calculator • How many hydrogen atoms are in 2. 5 moles of water? (Analyze, plan, solve, check)

Molar Mass or Gram-Formula Mass (GFM) • The Mass of 1 mole (in grams) • Equal to the numerical value of the average atomic mass (get from periodic table) 1 mole of C atoms = 12. 0 g 1 mole of Mg atoms = 24. 3 g 1 mole of Cu atoms = 63. 5 g

Other Names Related to Molar Mass or Gram-Formula Mass (GFM) • Molecular Mass/Molecular Weight: If you have a single molecule, mass is measured in amu’s instead of grams. But, the molecular mass/weight is the same numerical value as 1 mole of molecules. Only the units are different. (This is the beauty of Avogadro’s Number!) • Formula Mass/Formula Weight: Same goes for compounds. But again, the numerical value is the same. Only the units are different. • THE POINT: You may hear all of these terms which mean the SAME NUMBER… just different units

Learning Check! Find the molar mass or gram-formula mass (usually we round to the tenths place) A. 1 mole of Br atoms = B. 1 mole of Sn atoms = 79. 9 g/mole 118. 7 g/mole

Practice Problems – use mole road map or concept map to help you solve • How many atoms of copper are there in a 3 gram sample of copper? (Interconverting mass and numbers of particles)

Problems involving Empirical Formulas and Molecular Formulas • • Resources: PPT POGIL Practice problems (in-class, chapter problem set, online practice quiz questions)

Chemical Formulas of Compounds • Formulas give the relative numbers of atoms or moles of each element in a formula unit - always a whole number ratio (the law of definite proportions). NO 2 2 atoms of O for every 1 atom of N 1 mole of NO 2 2 mol of O atoms to every 1 mol of N atoms • If we know, or can determine, the relative number of moles of each element in a compound, we can determine a formula for the compound.

Types of Formulas • Empirical Formula The formula of a compound that expresses the smallest whole number ratio of the atoms present. Ionic formula are always empirical formula • Molecular Formula The formula that states the actual number of each kind of atom found in one molecule of the compound.

To obtain an Empirical Formula 1. Determine the mass in grams of each element present, if necessary. 2. Calculate the number of moles of each element. 3. Divide each by the smallest number of moles to obtain the simplest whole number ratio. 4. If whole numbers are not obtained* in step 3), multiply through by the smallest number that will give all whole numbers * Be careful! Do not round off numbers prematurely

A sample of a brown gas, a major air pollutant, is found to contain 2. 34 g N and 5. 34 g O. Determine a formula for this substance. require mole ratios so convert grams to moles of N = 2. 34 g of N = 0. 167 moles of N 14. 01 g/moles of O = 5. 34 g 16. 00 g/mole Empirical Formula: = 0. 334 moles of O

Calculation of the Molecular Formula A compound has an empirical formula of NO 2. The colourless liquid, used in rocket engines has a molar mass of 92. 0 g/mole. What is the molecular formula of this substance?

Empirical Formula from % Composition A substance has the following composition by mass: 60. 80 % Na ; 28. 60 % B ; 10. 60 % H What is the empirical formula of the substance? • Consider a sample size of 100 grams • This will contain 28. 60 grams of B and 10. 60 grams H • Determine the number of moles of each element • Determine the simplest whole number ratio of each element

Determination of Empirical Formulas using combustion analysis data for organic compounds • Experimental method that uses the mass of starting materials and masses of water and carbon dioxide produced to solve for the emp. Formula of organic compounds. • Steps?

Predicting Quantities of Products Based on Quantities of Reactants Use (use concept/road map) Grams of reactant (Given) Moles of reactant Moles of product Grams of product (To Find_

How do we do this? • Predicting Quantities of Products Based on Quantities of Reactants • Start from a balanced equation • Use concept/road map • Use dimensional analysis with (a) molar mass/ GFM and (b) mole ratios as the basis of conversion factors

Practice Problem (Practice ex. P. 103). The decomposition of potassium chlorate is commonly used to prepare small amounts of oxygen gas in the laboratory. How many grams of oxygen gas can be prepared from 4. 50 g of potassium chlorate?

Limiting reagents(reactants) problems (Start with POGIL “Limiting reactants”) • Start with the balanced chemical equation • Determine moles of reactants • Setup tables [(initial, change and end (final)] or ICE charts • Identify the limiting reagent/reactant • Finish the problem using dimensional analysis

Activities and Problem set X TB ch. 3 – all sections required for regents, SAT II and AP exams POGIL activities on chemical reaction equations, limiting reactants, etc Lab activities: • • • Determination Cux. Oy formula Percent composition of water in a hydrate Others - TBD Road/Concept map (provided) Online practice quiz due by ______ • Ch 3 Problems TO DO: write out questions and answers & show work • all GIST, sample & practice exercises, Visualizing concepts, • end of chapter 3 exercises: 10, 11 (b, e, g), 12 (d, g), 14, 15, 17, 19, 23 (b, d), 26 d, 27, 29, 33, 35, 37, 41, 43, 47, 53, 59, 63, 67, 68, 71, 73, 75, 80, 105