STOICHIOMETRY Molar mass Percent composition Moles Conversions Empirical

THE MOLE SI unit for amount A counting unit for measuring large quantities of

MOLAR MASS The amount of mass (grams) in one mole of a substance For

STEPS TO SOLVE 1. Find elements on periodic table 2. Write down the mass

SAMPLE: DETERMINE MOLAR MASS 1. Ca 1. 40. 08 g/mol Calculation s are FUN!

MOLAR MASS (CONT. ) 4. Fe 2 O 3 5. Na 2 O Fe:

PERCENT COMPOSITION Steps to solve 1. Find the total mass of the COMPOUND 2.

SAMPLE: CALCULATE THE PERCENT COMPOSITION CO 2 . 2730 100 27. 3 % .

SAMPLE 2 H 2 SO 4 H: (2)1. 008 g/mol = 2. 016 g/mol

COMPOSITION OF HYDRATES Hydrate: crystal contains water within • Water can fit into the

That was nothing. Time for Coco! SAMPLE PROBLEM: HYDRATE . 361 100 36. 1%

THE MOLE CONVERSION by Particles mo lar m 23 X b ma y Mol

STOICHIOMETRIC CONVERSIONS: MASS TO MOLES • You can relate any unit to another by

EXAMPLE How many moles are in 28 grams of CO 2? 28 grams CO

EMPIRICAL FORMULA • When the elements are in the smallest whole number ratio within

EXAMPLE: WHAT’S MY EMPIRICAL FORMULA 1. C 6 H 6 1. CH 2. C

EXAMPLE: WITH PERCENT A compound is found to contain 36. 48% Sodium, 25. 41%

MOLECULAR FORMULA Multiple of an empirical formula So many compounds with the same Empirical

STEPS TO SOLVE 1. Complete an empirical formula process if needed 2. Find the

All done! Time to go sledding! Yippee!! EXAMPLE C 4 H 4 O x

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STOICHIOMETRY Molar mass, Percent composition, Moles, Conversions, Empirical formulas, Molecular formulas 1

THE MOLE SI unit for amount A counting unit for measuring large quantities of small items Atoms molecules Particles 1 mole = 6. 022 x 10 23 atoms = molar mass 2

MOLAR MASS The amount of mass (grams) in one mole of a substance For elements Average atomic mass periodic table For compounds Must add up each element’s mass Subscripts are factored in by multiplication Units are g/mol May be called formula mass or molecular mass 3

STEPS TO SOLVE 1. Find elements on periodic table 2. Write down the mass 3. Multiply the mass by the subscript 4. Add together 4

SAMPLE: DETERMINE MOLAR MASS 1. Ca 1. 40. 08 g/mol Calculation s are FUN! 2. 55. 847 g/mol 2. Fe 3. Na. Cl Na: 22. 989 g/mol Cl: 35. 453 g/mol 58. 443 g/mol 5

MOLAR MASS (CONT. ) 4. Fe 2 O 3 5. Na 2 O Fe: 55. 847 x (2) = 111. 694 g/mol O: 15. 999 x (3)= 47. 997 g/mol 159. 691 g/mol Na: 22. 989 x(2) = 45. 978 g/mol O: 15. 999= 15. 999 g/mol 61. 977 g/mol 6

PERCENT COMPOSITION Steps to solve 1. Find the total mass of the COMPOUND 2. Take the mass of each element and divide it by the total mass 3. Multiply by 100 7

SAMPLE: CALCULATE THE PERCENT COMPOSITION CO 2 . 2730 100 27. 3 % . 727 100 72. 7% C: 12. 011 g/mol O: (2)15. 999 g/mol = 31. 998 g/mol 44. 009 g/mol 8

SAMPLE 2 H 2 SO 4 H: (2)1. 008 g/mol = 2. 016 g/mol S: 32. 064 g/mol O: (4)15. 999 g/mol = 63. 996 g/mol 98. 076 g/mol . 0206 100 2. 06 % . 327 100 32. 7 % . 653 100 65. 3% 9

COMPOSITION OF HYDRATES Hydrate: crystal contains water within • Water can fit into the salt crystal • Happens in fixed ratios • Each salt that forms a hydrate has a DIFFERENT water ratio • Each salt crystal is unique Anhydrous: water has been removed Steps to solve 1. Calculate the total mass of the compound INCLUDING THE water 2. Divide the water mass by total mass 3. Multiply by 100 • Achieved through drying 10

That was nothing. Time for Coco! SAMPLE PROBLEM: HYDRATE . 361 100 36. 1% H 2 O 11

THE MOLE CONVERSION by Particles mo lar m 23 X b ma y Mol ar ss ass 10 x 2 2 Mole . 0 6 y X b 3 2 2 0 6. ÷ by 2 10 Ions Atoms Molecules Formula units x x by 22. 4 L ÷ Mass (grams) Volume (Liters) Gases at STP 1 2

STOICHIOMETRIC CONVERSIONS: MASS TO MOLES • You can relate any unit to another by this method • Relate one unit to another • conversion factors Steps to convert 1. Identify what you start with 2. Determine what units you end in A. Might have to do side calculations 3. Set up conversion factor 4. Evaluate A. Do the Math! 1 3

EXAMPLE How many moles are in 28 grams of CO 2? 28 grams CO 2 . 636 _______ moles CO 2 C: 12. 011 g/mol O: (2)15. 999 g/mol = 31. 998 g/mol 44. 009 g/mol 14

EMPIRICAL FORMULA • When the elements are in the smallest whole number ratio within compound Steps to solve • When given a compound • Divide out by the common multiple Steps to solve • When given percentages 1. Change percent sign to grams (NO MATH) 2. Convert masses to moles A. Using conversions 3. Re-divide ALL moles amounts by the smallest mole amount A. Multiply if not whole numbers 4. Write compound with subscripts 15

EXAMPLE: WHAT’S MY EMPIRICAL FORMULA 1. C 6 H 6 1. CH 2. C 8 H 18 Piece of Cake! 2. C 4 H 9 3. C 2 H 6 O 2 3. CH 3 O 4. X 39 Y 13 4. X 3 Y 1 6

EXAMPLE: WITH PERCENT A compound is found to contain 36. 48% Sodium, 25. 41% Sulfur, and 38. 11% Oxygen. Find its empirical formula. Elemen t Percent Mass Na 36. 48% 36. 48 g 2 S 25. 41% 25. 41 g 1 O 38. 11 % 38. 11 g 3 Na 2 SO 3 Convert to moles Re-divide Subscript s 1 7

MOLECULAR FORMULA Multiple of an empirical formula So many compounds with the same Empirical formula 1

STEPS TO SOLVE 1. Complete an empirical formula process if needed 2. Find the mass of the EMPIRICAL FORMULA 3. Divide the Empirical formula mass by the molecular mass A. Molecular mass is normally given in the problem B. Answer is the common multiple 4. Multiple the SUBSCRIPTS by the common multiple 1 9

All done! Time to go sledding! Yippee!! EXAMPLE C 4 H 4 O x 2 = C 8 H 8 O 2 2 0