Percent Composition, Empirical and Molecular Formulas
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1 Percent Composition, Empirical and Molecular Formulas Chemists create new compounds for industry, pharmaceutical, and home use Analytical chemist analyzes new compound to provide proof of composition and chemical formula. Ex: Aspirin- C9H8O4
2 Percent Composition: the percent by mass of each element in a compound mass of element mass of compound x 100 = percent by mass *If given mass of each element--just divide. Example: A compound was found to contain 49.98g C and 10.47g H. What is the percent composition?
3 Given the chemical formula, to find the percent composition Assume you have 1 mole of the compound 2. Find the mass of each element (molar mass x subscript) 3. Use formula for percent by mass
4 Example 1: Find the percent composition of H2O February 26, 2014
5 Example 2: Find the percent composition of sodium hydrogen carbonate (NaHCO3, or baking soda) February 26, 2014
6 For a new compound, if the elements in a sample are known and the percent composition is known, we can find the formula of the compound. 1. Find empirical formula 2. Find molecular formula
7 Empirical Formula: Smallest whole number ratio of moles of elements in the compound determines subscripts may or may not be the same as molecular formula For example: The empirical formula of hydrogen peroxide is HO (H1O1) The molecular formula of hydrogen peroxide is H2O2
8 How to find empirical formula... If you are given the percent composition in a given mass of compound Assume you have 100g of the compound > Percent by mass = mass of element 2. Convert each mass to moles 3. If the moles are not whole numbers, divide the moles by the smallest mole of an element 4. If still not whole numbers, multiply by smallest number to produce a ratio of whole numbers *If you are given the mass of each element, start at step 2.
9 Example 3: Percent composition of an oxide of sulfur is 40.05% S and 59.95% O 1. Assume you have 100g of the compound > Percent by mass = mass of element 2. Convert each mass to moles 3. If the moles are not whole numbers, divide the moles by the smallest mole of an element 4. If still not whole numbers, multiply by smallest number to produce a ratio of whole numbers
10 Example 4: Determine the empirical formula of methyl acetate which has the collowing percent composition: 48.64% C, 8.16% H, and 43.20% O February 26, 2014
11 Molecular Formula: specified actual number of each element in one molecule *Different substances (different molecular formulas) can have the same empirical formula. Ex: Acetylene and Benzene both have the empirical formula CH Acetylene: C2H2 Benzene: C6H6
12 To determine the molecular formula for a compound Take the experimentally determined molar mass (will be given to you) 2. Divide by mass of empirical formula ***This will tell you how many times bigger the molar mass is*** 3. Multiply empirical formula by result.
13 Example 5: What is the molecular formula of succinic acid? The molar mass of succinic acid is 118.1g/mol. The empirical formula is C2H3O2 1. Take the experimentally determined molar mass (will be given to you) 2. Divide by mass of empirical formula ***This will tell you how many times bigger the molar mass is*** 3. Multiply empirical formula by result.
14 Example 6: A compound was found to contain 49.98g C and 10.47g H. The molar mass is 58.12g/mol. Determine the molecular formula. February 26, Determine empirical formula 2. Determine molecular formula
15 Example 7: A colorless liquid composed of 46.68% N and 53.32% O has a molar mass of 60.01g/mol. What is the molecular formula?
16 February 26, 2014 Hydrate: A compound that has a specific number of water molecules bound to its atoms. Example: Opal (a gemstone) is composed of Silicon dioxide ( ). The coloring is the result of water in the mineral.
17 February 26, 2014 Hydrate: A compound that has a specific number of water molecules bound to its atoms. Example: Desiccants--anhydrous (w/o water) form of hydrate can absorb water from air
18 Hydrates A formula for a hydrate indicates the # of water molecules associated with the formula of the compound > Example: Na2CO3 10H2O (Sodium carbonate decahydrate)
19 To determine the formula for a hydrate Find moles of water associated with 1 mole of hydrate > Mass hydrate compound > Heat sample of hydrate to drive off water > Mass anhydrous (w/o water) compound > Find difference:massh2o=masshydrate - Massanhydrous 2. Find moles of water 3. Find moles of anhydrous compound 4. Calculate ratio of moles of water to compound moles water moles anhydrous compound
20 Example 8: A mass of 2.50g of hydrated copper sulfate (CuSO4 xh2o) is heated. After heating, 1.59g anhydrous copper sulfate (CuSO4) remains. what is the formula of the hydrate? 1. Find moles of water associated with 1 mole of hydrate > Mass hydrate compound > Heat sample of hydrate to drive off water > Mass anhydrous (w/o water) compound > Find difference:mass H2O= Mass hydrate - Mass anhydrous 2. Find moles of water 3. Find moles of anhydrous compound 4. Calculate ratio of moles of water to compound moles water moles anhydrous compound
21 Example 9: A mass of 11.75g of hydrated cobalt (II) chloride is heated. After heating, 9.25g anhydrous cobalt (II) chloride remains. what is the formula of the hydrate? 1. Find moles of water associated with 1 mole of hydrate > Mass hydrate compound > Heat sample of hydrate to drive off water > Mass anhydrous (w/o water) compound > Find difference:mass H2O= Mass hydrate - Mass anhydrous 2. Find moles of water 3. Find moles of anhydrous compound 4. Calculate ratio of moles of water to compound moles water moles anhydrous compound
22 Example 10: A hydrate is found to have the following percent composition: 48.8% MgSO4 and 51.2% H2O. What is the formula and name for this hydrate? *Hint: Think about what percent composition means! Look back on how to find empirical formula from percent composition
23
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= 16.00 amu. = 39.10 amu
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IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
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b. N 2 H 4 c. aluminum oxalate d. acetic acid e. arsenic PART 2: MOLAR MASS 2. Determine the molar mass for each of the following. a. ZnI 2 b.
CHEMISTRY DISCOVER UNIT 5 LOTS OF PRACTICE ON USING THE MOLE!!! PART 1: ATOMIC MASS, FORMULA MASS, OR MOLECULAR MASS 1. Determine the atomic mass, formula mass, or molecular mass for each of the following
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