Proust Law Review
diana.aguascs
Created on April 8, 2021
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Transcript
April 2021Profesor Diana Aguas Chantes
Proust's Law of Definite Proportions
Joseph Proust
In other words, the ratios of the elements included are always the same, no matter the total amount of the compund.
"A chemical compound always contains the same elements combined together in the same proportion by mass."
Water, H2O.
EXAMPLE:
11.11 % corresponds to g Hydrogen, and the other 88.89% to Oxygen.
Percentages
The mass is negligible, if you consider that you'll always get a compound formed at its 100% no matter how many grams reacted.
But
1 atom of Oxygen and 2 atoms of Hydrogen
H2O
16 g of Oxygen and 2 g of Hydrogen
One molecule of water
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Exercise 1
If the percentages of N and H in ammonia (NH3) are respectively 82.40% and 17.60%. Determine the mass of ammonia that can be obtained from 10 g of N and 6 g of hydrogen.
4. We see now that by having 10 g of Nitrogen, only 2.136 g of H will react, therefore H is in excess.5. Adding up: 2.136 g + 10 g = 12.136 g of NH3
Exercise 1
1. Remember the reaction does not depend on the mass but on the proportions.2. By taking masses randomly, it is likely that one of the two components will be in excess and the other on will be limited.3. Apply Sandwich Rule:
If the percentages of N and H in ammonia (NH3) are respectively 82.40% and 17.60%. Determine the mass of ammonia that can be obtained from 10 g of N and 6 g of hydrogen.
At certain conditions, sulfur and sodium will react to form sodium sulfide. Hence, 4.60 g of sodium originate 7.80 g of sulfide. How much sulfur will be combined with 15 g of sodium?
Exercise 2
1. Taking into account Lavoisier's law, we obtain the amount of sulfur in the compound:2. Following Proust's Law:
https://www.youtube.com/watch?v=08-96_wkUi8&t=1s
https://chemistrygod.com/law-of-definite-proportions
Consulted material