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Vocabulary Percent Composition -
Tells you the percentage of the mass made up by each element in the compound Empirical Formula - Gives the simplest whole number ratio of the atoms of the element Molecular Formula - Gives actual number of atoms of each element in the molecular compound
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Calculating Percent Composition
% of element = mass of element x formula mass compound Example What is the percent composition of hydrogen and oxygen in water? Chemical Formula = H2O Formula mass = 2( g) g = g % of H = g x g = 11.2% % of O = 100 – = 88.8%
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Example. Find the percent composition of a compound. that contains 2
Example Find the percent composition of a compound that contains 2.30g Na, 1.60g O and 0.100g H . Total mass = 2.30g g g = 4.00g % of Na = g x g = % % of O = g x g = % % of H = g x g = 2.5 %
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Example. A sample of an unknown compound with a. mass of 0
Example A sample of an unknown compound with a mass of 0.562g has the following percent compositions: 13.0% C, 2.2% H and 84.8% F. What is the mass of each element? Formula mass = % of C = mass C x g = % Mass C = g % of H = mass H x g = 2.2 % Mass H = g % of F = mass F x g = % Mass F = 0.477g
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Vocabulary Percent Composition -
Tells you the percentage of the mass made up by each element in the compound Empirical Formula - Gives the simplest whole number ratio of the atoms of the element Molecular Formula - Gives actual number of atoms of each element in the molecular compound
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Calculating Percent Composition
% of element = mass of element x formula mass compound Example What is the percent composition of hydrogen and oxygen in water? Chemical Formula = H2O Formula mass = 2( g) g = g % of H = g x g = 11.2% % of O = 100 – = 88.8%
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Example. Find the percent composition of a compound. that contains 2
Example Find the percent composition of a compound that contains 2.30g Na, 1.60g O and 0.100g H . Total mass = 2.30g g g = 4.00g % of Na = g x g = % % of O = g x g = % % of H = g x g = 2.5 %
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Example. A sample of an unknown compound with a. mass of 0
Example A sample of an unknown compound with a mass of 0.562g has the following percent compositions: 13.0% C, 2.2% H and 84.8% F. What is the mass of each element? Formula mass = % of C = mass C x g = % Mass C = g % of H = mass H x g = 2.2 % Mass H = g % of F = mass F x g = % Mass F = 0.477g
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