Your SlideShare is downloading. ×
Chemistry 30S Unit 3 – Chemical Reactions
<ul><li>Recall that in a  chemical  formula, the elements are represented by symbols and a subscript represents the number...
<ul><li>An  empirical  (Simplest) formula represents the relative number of atoms of each element in the compound </li></u...
<ul><li>The percent composition of a compound is the mass of each element divided by the total mass of the compound x 100%...
<ul><li>Example Problem </li></ul><ul><li>Experimental analysis determined that a compound contained 7.30g of sodium, 5.08...
<ul><li>Example Problem </li></ul><ul><li>If a compound has a composition of 40.0% carbon, 6.71% hydrogen and 53.29% oxyge...
<ul><li>Example Problem </li></ul><ul><li>If a compound contains 71.65% chlorine, 24,27% carbon, and 4.07%hydrogen, determ...
Upcoming SlideShare
Loading in...5
×

% Composition

1,340

Published on

Published in: Education, Technology
0 Comments
0 Likes
Statistics
Notes
  • Be the first to comment

  • Be the first to like this

No Downloads
Views
Total Views
1,340
On Slideshare
0
From Embeds
0
Number of Embeds
1
Actions
Shares
0
Downloads
0
Comments
0
Likes
0
Embeds 0
No embeds

No notes for slide

Transcript of "% Composition"

  1. 1. Chemistry 30S Unit 3 – Chemical Reactions
  2. 2. <ul><li>Recall that in a chemical formula, the elements are represented by symbols and a subscript represents the number of each element </li></ul>CHEMICAL REACTIONS Chemical - Empirical - Molecular Formulas C 2 H 6
  3. 3. <ul><li>An empirical (Simplest) formula represents the relative number of atoms of each element in the compound </li></ul><ul><ul><li>C 2 H 6 becomes CH 3 </li></ul></ul><ul><li>A molecular formula represents the actual number of atoms of each element rather than a ratio of atoms. </li></ul><ul><ul><li>C 2 H 6 </li></ul></ul><ul><ul><li>Molecular Formula = Empirical Formula x n </li></ul></ul>CHEMICAL REACTIONS Chemical - Empirical - Molecular Formulas
  4. 4. <ul><li>The percent composition of a compound is the mass of each element divided by the total mass of the compound x 100%. </li></ul><ul><li>The percent composition can be determined from the formula or experimentally by a decomposition reaction. </li></ul>CHEMICAL REACTIONS Percent Composition C 2 H 6
  5. 5. <ul><li>Example Problem </li></ul><ul><li>Experimental analysis determined that a compound contained 7.30g of sodium, 5.08g of sulphur, and 7.62g of oxygen. What is the simplest formula of this compound. </li></ul><ul><li>Solution: </li></ul>CHEMICAL REACTIONS Percent Composition M
  6. 6. <ul><li>Example Problem </li></ul><ul><li>If a compound has a composition of 40.0% carbon, 6.71% hydrogen and 53.29% oxygen, determine the empirical formula of the compound. </li></ul><ul><li>Solution: </li></ul><ul><li>Assume that there is a 100.0g sample in this case: </li></ul>CHEMICAL REACTIONS Percent Composition
  7. 7. <ul><li>Example Problem </li></ul><ul><li>If a compound contains 71.65% chlorine, 24,27% carbon, and 4.07%hydrogen, determine the molecular formula if the molar mass is 98.96g/mol. </li></ul><ul><li>Solution: </li></ul><ul><li>Assume that there is a 100.0g sample in which case: </li></ul>CHEMICAL REACTIONS Percent Composition

×