Percent Composition
Percent Review <ul><li>Any percentage calculation involves a portion/part of the total over the total </li></ul>
Review <ul><li>% concentration =  </li></ul>
Review <ul><li>% concentration = </li></ul>Grams of solute Grams of solution
<ul><li>% concentration = </li></ul>Review Grams of solute Grams of solution X 100
Percent Composition <ul><li>The percent by mass of each element found in a compound. </li></ul>Mass of element Mass of com...
Example <ul><li>Water = H 2 O </li></ul>
Example <ul><li>Water = H 2 O </li></ul><ul><ul><li>2 hydrogens (mass = 1.0 each) </li></ul></ul><ul><ul><li>1 oxygen (mas...
Example <ul><li>Water = H 2 O </li></ul><ul><ul><li>2 hydrogens (mass = 1.0 each) </li></ul></ul><ul><ul><li>1 oxygen (mas...
Example <ul><li>Water = H 2 O </li></ul><ul><li>Mass of oxygen </li></ul><ul><li>Mass of water </li></ul>
Example <ul><li>Water = H 2 O </li></ul><ul><li>Mass of oxygen </li></ul><ul><li>Mass of water </li></ul><ul><li>16.0 </li...
Recap <ul><li>A percentage is a ratio of part : whole </li></ul><ul><li>Percent composition is the ratio of an element’s m...
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Percent composition

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Percent composition

  1. 1. Percent Composition
  2. 2. Percent Review <ul><li>Any percentage calculation involves a portion/part of the total over the total </li></ul>
  3. 3. Review <ul><li>% concentration = </li></ul>
  4. 4. Review <ul><li>% concentration = </li></ul>Grams of solute Grams of solution
  5. 5. <ul><li>% concentration = </li></ul>Review Grams of solute Grams of solution X 100
  6. 6. Percent Composition <ul><li>The percent by mass of each element found in a compound. </li></ul>Mass of element Mass of compound X 100 = percent composition
  7. 7. Example <ul><li>Water = H 2 O </li></ul>
  8. 8. Example <ul><li>Water = H 2 O </li></ul><ul><ul><li>2 hydrogens (mass = 1.0 each) </li></ul></ul><ul><ul><li>1 oxygen (mass = 16.0) </li></ul></ul>
  9. 9. Example <ul><li>Water = H 2 O </li></ul><ul><ul><li>2 hydrogens (mass = 1.0 each) </li></ul></ul><ul><ul><li>1 oxygen (mass = 16.0) </li></ul></ul><ul><li>2 hydrogens @ 1.0  2 X 1.0 = 2.0 </li></ul><ul><li>1 oxygen @ 16.0  1 X 16.0 = 16.0 </li></ul><ul><li>Total = 18.0 </li></ul>
  10. 10. Example <ul><li>Water = H 2 O </li></ul><ul><li>Mass of oxygen </li></ul><ul><li>Mass of water </li></ul>
  11. 11. Example <ul><li>Water = H 2 O </li></ul><ul><li>Mass of oxygen </li></ul><ul><li>Mass of water </li></ul><ul><li>16.0 </li></ul><ul><li>18.0 </li></ul>X 100 = 89.9 %
  12. 12. Recap <ul><li>A percentage is a ratio of part : whole </li></ul><ul><li>Percent composition is the ratio of an element’s mass to the total mass of the compound </li></ul>Mass of element Mass of compound X 100 = percent composition
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