% Composition, Empirical Formulas, & Molecular Formulas.
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Transcript of % Composition, Empirical Formulas, & Molecular Formulas.
![Page 1: % Composition, Empirical Formulas, & Molecular Formulas.](https://reader036.fdocuments.in/reader036/viewer/2022082418/5697bf891a28abf838c89f06/html5/thumbnails/1.jpg)
% Composition, Empirical Formulas, & Molecular Formulas
![Page 2: % Composition, Empirical Formulas, & Molecular Formulas.](https://reader036.fdocuments.in/reader036/viewer/2022082418/5697bf891a28abf838c89f06/html5/thumbnails/2.jpg)
% Composition
• % = (part / whole ) x 100
• When calculating the % composition, you are calculating the % of each element in a compound
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% Composition
• Calculate the % Composition of MgO
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% Composition
• Calculate the % Composition of iron (III) oxide
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Empirical & Molecular Formulas
• Empirical formula – the ____________ whole number ratio of elements
• Molecular formula – the ____________ number of elements in a compound
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Empirical Formula
• What is the empirical formula for H2O2?
• What is the empirical formula for C6H12O6?
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Steps for Calculating the Empirical Formula
1. List your givens
2. Change % to grams
3. Change grams to moles
4. Divide everything by the smallest number of moles
5. Write your formula
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Empirical Formula Problem
• Calculate the empirical formula of a compound containing 40.05 % S and 59.95 % O.
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Empirical Formula Problem
• Calculate the empirical formula for a compound containing 48.64 g C, 8.16 g H, and 43.20 g O.
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Steps for Calculating Molecular Formula
1. Calculate the ____________
2. Get the ____________ of the empirical formula that you just determined
3. Divide the ____________ by the molecular mass of the empirical formula
4. You will get a whole number
5. Multiply everything in the empirical formula by this number
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Molecular Formula Problem
• Calculate the molecular formula of a compound containing 40.68%C, 5.08%H, and 54.25%O with an experimentally determined molecular weight of 118.1 g/mol
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Molecular Formula Problem
• Calculate the molecular formula of a compound containing 57.84 g C, 3.64 g H, and 38.52 g O with an experimentally determined molecular mass of 249.21 g/mol
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Empirical Formula with Combustion Data Steps
1.Calculate the number of grams of carbon
2.Calculate the % C
3.Calculate the number of grams of hydrogen
4.Calculate the % H
5.Calculate the % of any other element by subtracting % C & % H from 100.
6.Continue the empirical formula calculation as usual
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Example
• A compound is comprised of carbon, hydrogen, and nitrogen. When 0.1156 g of this compound is reacted with oxygen, 0.1638 g of CO2 and 0.1676 g of water are collected. Assuming that all of the carbon in the compound is converted into CO2, determine the empirical formula of the compound.
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Another example
• A 0.3410 g sample of a carbon-hydrogen-oxygen hydrocarbon was combusted to produce 0.7500 g CO2 and 0.1363 g H2O. The molecular mass was determined to be 180 g/mol. Determine the empirical and molecular formulas of the compound.
• Both the empirical and molecular formulas are C9H8O4.
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One more example
• A 0.821 g hydrocarbon sample was combusted to yield 1.866 g CO2 and 0.7639 g H2O. The molecular mass was determined to be 116 g/mol. Determine the empirical and molecular formulas of the compound.
• C3H6O is empirical formula
• C6H12O2 is molecular formula
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