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Lavoisier's Conservation of Mass Experiment
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Lavoisier's Conservation of Mass
Background
Chemistry was not yet acknowledged as a true science. The original elements, earth, air, water, and fire, presented by Aristotle had been slowly refined by alchemists. There was a theory called ‘phlogiston’ developed by Georg Ernst Stahl early in the 18th century. It was easily accepted because it seemed to explain so much in a simple fashion.
Definition
phlogiston-
a universal component of fire that was thought to be contained in every combustible substance, lost to the air when burned
Purpose
Purpose & Hypothesis
Lavoisier learned about the concept of phlogiston during college, and become interested in combustion. He performed experiments that had results that could not be explained by the theory, and took to find out why. Ultimately, his purpose was to disprove and figure out the truth behind Stahl’s development of phlogiston.
Hypothesis
Lavoisier believed that air was not a simple substance and that it actually had 2 components- one that combined with metal and supported respiration, and one that did not support combustion or respiration. He completely disagreed with Stahl and claimed that
“phlogiston is imaginary.”
Experiments
Experiments & Variables
He experimented with phosphorus, sulfur, mercury and lead calx, oxygen, water, hydrogen, and many different elements. Before conducting, he carefully analyzed the properties of metals and designed a series of experiments that allowed him to measure not just the mass of the metal but also the mass of the air surrounding the reaction.
Variables
The independent variable was the element that Lavoisier was burning, the dependent variable would be the end result, the calx.
Constants included the weight, the method of burning, location, and air quality.
Data
Data & Conclusion
After Lavoisier's experiment, he proposed that combustion was the reaction of a substance with "common air." He called it oxygène from the 2 Greek words for acid generator. In 1789 he published the Elements of Chemistry textbook. It included information on chemical reactions, gases, acids and bases, and defined the Law of the Conservation of Mass.
Conclusion
Law of Conservation of Mass: mass is neither created nor destoryed by chemical reactions; the amount of matter cannot change.
Results
Lavoisier declared his findings to the Royal Academy of Sciences in Paris, shared results with colleagues, published his own book, wrote the Law of Conservation of Mass and the Table of Simple Substances.