Question

show that the law of constant proportion is a necessary consequences of atomic theory​

Answer 1

Answer:

When you work with chemistry problems using this law, your goal is to look for the closest mass ratio between the elements. It's okay if the percentage is few hundredths off! If you're using experimental data, the variation might be even larger.

For example, let's say you want to demonstrate, using the law of constant composition that two samples of cupric oxide abide by the law. The first sample was 1.375 g cupric oxide, which was heated with hydrogen to yield 1.098 g of copper. For the second sample, 1.179 g of copper was dissolved in nitric acid to produce copper nitrate, which was then burned to produce 1.476 g of cupric oxide.

To work the problem, you need to find the mass percent of each element in each sample. It doesn't matter whether you choose to find the percent of copper or of oxygen. You would just subtract one value from 100 to get the percent of the other element.

Write down what you know:

In the first sample:

copper oxide = 1.375 g

copper = 1.098 g

oxygen = 1.375 - 1.098 = 0.277 g

percent oxygen in CuO = (0.277)(100%)/1.375 = 20.15%

For the second sample:

copper = 1.179 g

copper oxide = 1.476 g

oxygen = 1.476 - 1.179 = 0.297 g

percent oxygen in CuO = (0.297)(100%)/1.476 = 20.12%

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