Understanding the Law of Multiple Proportions
The Law of Multiple Proportions states that when two elements form more than one compound, the ratios of the masses of one element that combine with a fixed mass of the other element are simple whole numbers.
Analyzing the Data
* Higher Oxide: We are told that the higher oxide contains 80% metal. This means that for every 100 grams of the oxide, 80 grams are metal, and the remaining 20 grams are oxygen.
* Lower Oxide:
* We start with 0.72 grams of the lower oxide.
* After oxidation, it becomes 0.8 grams. This means 0.08 grams of oxygen were added to the lower oxide.
* Since the metal in the lower oxide remains constant, we can deduce that the original 0.72 grams contained 0.72 - 0.08 = 0.64 grams of metal.
Calculating the Mass Ratios
Now, let's calculate the mass ratios of oxygen to metal in each oxide:
* Higher Oxide: Oxygen/Metal = 20/80 = 1/4
* Lower Oxide: Oxygen/Metal = 0.08/0.64 = 1/8
Applying the Law of Multiple Proportions
Notice that the ratio of oxygen to metal in the higher oxide (1/4) is exactly twice the ratio of oxygen to metal in the lower oxide (1/8).
This confirms the Law of Multiple Proportions: The masses of oxygen that combine with a fixed mass of metal in the two oxides are in a simple whole number ratio (1:2).
Conclusion
The given data perfectly illustrates the Law of Multiple Proportions. The two oxides of the metal demonstrate that the ratio of the mass of oxygen combining with a fixed mass of the metal is a simple whole number ratio (1:2).
