# Study About Law of Multiple Proportions with Examples and Limitations

## Abstract

The basic objective of this study is to illustrate the Law of multiple proportions. The basic purpose of Dalton law to express this law is to simply to aware this world about the chemistry world.

And importantly to find out the real reason how two elements combine with the same form and the masses of these elements change with this time passage.

## Definition Law of Multiple proportions

People usually believed in that thing Dalton proposed that particular law investigate or express the validity of Atomic theory. Subsequently this law and Atomic theory interlinked.

The law of multiple proportions definition defines as when two elements form produced any compound by interlinked with each other. Then the mass ratio of the 2nd elements turns into the small whole number.

When John Dalton discovers this law, people treat it like a Dalton hypothesis model only.

But the thing is Atomic theory is a key proof of discovering this model.

## Example

• Law of multiple proportions example included the following things.
• Let’s suppose we consider that 100 grams of carbon, may interlink with 133 grams of oxygen to produce the other compound. Or 266 grams’ oxygen required to produce one oxide. So the ratios of these masses will be 1:2.
• Oxygen and carbon combine with each other to produce another compound with a small whole number. Either it will take 1 element or either it will take 2 elements of oxygen to react with the carbon.
• The other example is that we compare the ethane and propane proportions to form another compound.
•  we figured this thing out that 1 g carbon is equal to .252 of ethane and .242 of propane which formulated the small whole numbers ratios as 9:8. ## Limitations

• The law of multiple proportions is not widely true or acceptable. In the above- example’s we found that the law is only applicable to small Reactions.
• It means that this law is valid for tiny chemical reactions.
• The Law of multiple proportions is not valid for heavy molecules
• Because when heavy molecules interlinked with each other than the total whole will not be as small.

There are some google questions that people usually search to clear their doubts. So we will discuss it one by one.

## What is the Law of Multiple Proportions?

interlinking of two compounds to form a new compound in between with a small whole number.

## Which set of compounds illustrates the law of multiple proportions?

Let’s take an example it does not apply to So2 and Co2. The reason behind this concept is that these are two different compounds.

N2O4 and N2O is a perfect example of this concept. Because both compounds are the same with equal molecules.

## Which of the following pairs of compounds can be used to illustrate the law of multiple proportions?

• Water(H2o) and Hydrogen peroxide(H2o2) is a paired example of this law.

## Which pair of substances could be used to illustrate the law of multiple proportions?

• CO (Carbon monoxide) and Co2 (Carbon dioxide)  substances used to express this law.

## Which of the following is an example of the law of multiple proportions?

Water and hydrogen peroxide plus carbon and carbon dioxide are the main examples of this concept.

For this there is only one rule whosever substances have the same compound will generate the whole small number. But there will be no small whole number if two heavy atomic compounds will be interlinked with each other.

## Conclusion

In the conclusion, we must say that the law of multiple proportions is a study of the chemistry field. it is presented by john dalton for investigating the validity of Atomic theory. Most of the Authors disagree with that law because this specifically applies to normal reactions.

There are some examples that also included in this Article and some limitations as well.

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