Justify the law of multiple proportion by taking the example of combination between C and O to form CO and CO2
Answers
Law of Multiple proportion states that when two elements combine to form more than one compound, the mass of one element, which combines with a fixed mass of the other element, will always be ratios of whole numbers.
For example, let us assume 2 molecules CO (carbon monoxide) and CO
2
(carbon dioxide).
CO= 12gm of carbon + 16 grams of Oxygen.
CO
2
= 12gm carbon+ 32 grams of Oxygen.
The ratio of the mass of oxygen in the given two compounds is 16:32=1:2.
Thus law of multiple proportions is proved.
Answer:
Once the idea that elements combined in definite proportions to form compounds was established, experiments also began to demonstrate that the same pairs of certain elements could combine to form more than one compound.
Consider the elements carbon and oxygen. Combined in one way, they form the familiar compound called carbon dioxide. In every sample of carbon dioxide, there is 32.0 g of oxygen present for every 12.0 g of carbon. By dividing 32.0 by 12.0, this simplifies to a mass ratio of oxygen to carbon of 2.66 to 1. There is another compound that forms from the combination of carbon and oxygen called carbon monoxide. Every sample of carbon monoxide contains 16.0 g of oxygen for every 12.0 g of carbon. This is a mass ratio of oxygen to carbon of 1.33 to 1. In the carbon dioxide, there is exactly twice as much oxygen present as there is in the carbon monoxide.
This example illustrates the law of multiple proportions: Whenever the same two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers.
Explanation:
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