Understanding the Law of Multiple Proportions
The Law of Multiple Proportions states that when two elements (in this case, the metal and oxygen) form more than one compound, the masses of one element that combine with a fixed mass of the other element are in a simple ratio of whole numbers.
Analyzing the Data
1. Higher Oxide: The higher oxide contains 80% oxygen by mass. This means that if we have 100g of the higher oxide, 80g of it is oxygen, and the remaining 20g is the metal.
2. Lower Oxide: We are given 0.72g of the lower oxide. Let's find the mass of oxygen and the metal in this sample.
* Mass of oxygen in lower oxide: To determine this, we need to know the percentage of oxygen in the lower oxide. We'll assume a variable 'x' represents the percentage of oxygen in the lower oxide.
* Mass of metal in lower oxide: 0.72g (total lower oxide) - (mass of oxygen in lower oxide) = mass of metal.
3. Oxidation of Lower Oxide: The 0.72g of lower oxide is oxidized to 0.8g of the higher oxide. This tells us that the metal in the lower oxide gains more oxygen to form the higher oxide.
Applying the Law
To demonstrate the Law of Multiple Proportions, we need to show that the masses of oxygen that combine with a fixed mass of the metal in the two oxides are in a simple ratio of whole numbers.
Let's assume a fixed mass of the metal in both oxides. For simplicity, we'll assume the metal's mass is 1g.
* Higher Oxide:
* Mass of oxygen: 80% of 100g = 80g (for a 100g sample)
* Mass of metal: 20g (for a 100g sample)
* Since we are assuming 1g of metal, the mass of oxygen in the higher oxide is (80g / 20g) * 1g = 4g.
* Lower Oxide:
* We need to calculate the mass of oxygen in the 0.72g sample. To do this, we'll need to know the percentage of oxygen in the lower oxide (which we represented with 'x'). Let's assume we determine 'x' through further analysis of the data.
* Once we have the mass of oxygen in the lower oxide, we can calculate the ratio of oxygen masses between the two oxides for the same mass of the metal (1g in our example).
Conclusion
If we determine the mass of oxygen in the 0.72g sample of lower oxide and find that the ratio of oxygen masses in the two oxides is a simple ratio of whole numbers (e.g., 2:1, 3:2, etc.), then the data illustrates the Law of Multiple Proportions.
