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Ch 3.4 law of definite proportions 11 12

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Information about Ch 3.4 law of definite proportions 11 12

Published on February 21, 2014

Author: nikkiwwilkinson

Source: slideshare.net

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Law of Definite Proportions  Regardless of the amount, a compound is always composed of the same elements in the same proportion by mass.  The proportions are found by calculating the percent by mass.

Percent by Mass  Based on the law of conservation of mass MASS compd = sum of MASSES elements  % by mass = MASSelement x 100% MASScompd

Percent by Mass  Example on page 75  Sucrose = Carbon, hydrogen, oxygen  To find percent by mass of each element: C= (mass C / mass of sucrose) x 100% H= (mass H / mass of sucrose) x 100% O= (mass O / mass of sucrose) x 100%

Percent by Mass (20g of sucrose) Element Analysis by mass (g) Percent by mass (%) Carbon 8.4 8.4 x 100 = 42% 20.0 Hydrogen 1.3 1.3 x 100 = 6.5% 20.0 Oxygen 10.3 10.3 x 100 = 51.5% 20.0 Total (Sucrose) 20.0 100%

Percent by Mass (500g sucrose) Element Analysis by mass (g) Percent by mass (%) Carbon 210.5 210.5 x 100 = 42% 500.0 Hydrogen 32.4 32.4 x 100 = 6.5% 500.0 Oxygen 257.1 257.1 x 100 = 51.5% 500.0 Total (Sucrose) 500.0 100%

Law of Definite Proportions  Therefore, mass percentages of elements in a compound do NOT depend on amount.  Compounds with the same mass proportions must be the same compound

Practice Problems Q: A 78.0 g sample of an unknown compound contains 12.4g of hydrogen. What is the percent by mass of hydrogen in the compound? A: % Mass H = mass H x 100% mass comp = 12.4g x 100% 78.0g = 15.9%

Practice Problems Q: If 3.5 g of X reacts with 10.5g of Y to form the compound XY, what is the percent by mass of X in the compound? A: % Mass X = mass X x 100% mass XY = 3.5g (3.5 + 10.5)g = 25% x 100%

Practice Problems Q: If 3.5 g of X reacts with 10.5g of Y to form the compound XY, how many grams of Y would react to form XY2? A: Mass YXY = 2 ( Mass YXY ) 2 = 2 ( 10.5g) = 21.0 g

Practice Problems Q: 2 unknown compounds are tested. Compound 1 contains 15.0g of hydrogen and 120.0g oxygen. Compound 2 contains 2.0g of hydrogen and 32.0g oxygen. Are the compounds the same? HINT!! If % Masses = , then they are the same

Practice Problems A: Compd 1%H = = %O = = [15.0 / (15.0+120.0)] x 100% 11.1% [120.0 / (15.0+120.0)] x 100% 88.9% Compd 2%H = [2.0 / (2.0+32.0)] x 100% = 5.9% %O = [32.0 / (2.0+32.0)] x 100% = 94.1% NOT THE SAME COMPOUNDS

More Practice Complete #s 10 – 13 on page 28-29 of Solving Problems: A Chemistry Handbook.

More Practice (ANSWERS) 10. a) % Bromine = 72.9% b) Total = 100% 11. % Hydrogen = 4.48% % Carbon = 60.00% % Oxygen = 35.52% 12. % Sulfur = 33.6% % Copper = 66.4% 13. Mass of oxygen = 14.6g

Handout Key 1. 2. 3. 4. 5. 7. Since the mass percentages in the unknown compound are the same as in sucrose, the compound must be sucrose. Since amount does NOT affect mass percentages, the mass percentage of carbon is 42.40% in 5, 50, and 500 g of sucrose. 51.30% = [Mass O / 50.00g sucrose] x 100% Mass O = [51.30 / 100] x 50.00 = 25.65g 42.40% = [Mass C / 100.0g sucrose] x 100% Mass C = [42.40 / 100] x 100.0 = 42.40g 6.50% = [Mass H / 6.0 g sucrose] x 100% Mass H = [6.50 / 100] x 6.0 = 0.39g % Cl= [12.13g Cl / 20.00g salt] x 100% = 60.65% % Na= [7.87g Na / 20.00g salt] x 100% = 39.4%

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