Chemistry usually involves chemical reactions where two or more elements combine to produce a single compound. The reactions involving the combination of various elements to produce a single compound are governed by the 5 laws of chemical combination.
Let us understand what these five laws have to say about various chemical combinations taking place in nature.
The law of conservation of mass was proposed by Antonie Lavoisier in 1789 and was based on results obtained from various combustion reactions.
According to the law of conservation of mass, “mass can neither be created nor destroyed, it can only be transformed from one form to another”.
In chemistry, the law of conservation of mass states that the total mass of the product obtained by chemical combination is equal to the sum of the mass of all reactants involved.
Example - The heating of calcium carbonate (10grams) produces calcium oxide (5.6 grams) and calcium dioxide (4.4 grams).
According to the law of conservation of mass,
Total mass of reactants = Total mass of products
Mass of calcium carbonate = Mass of calcium oxide + Mass of carbon dioxide
10.0 grams = 5.6 grams + 4.4 grams
10.0 grams = 10.0 grams
Joseph Proust proposed the law of definite proportions in 1799. It is called Proust’s law or the law of constant proportions.
According to the law of definite proportions, elements are always combined in specific definite proportions only. It means that elements always combine in a specific ratio irrespective of the number of reactants taken or the source from which they were obtained.
Example - Ethyl alcohol (C2H5OH).
Irrespective of the total amount of ethyl alcohol present, its combination consists of 52% of carbon, 35% of oxygen, and 13% of hydrogen by weight. This is according to the law of constant proportions.
John Dalton proposed the law of multiple proportions in 1804.
According to the law of multiple proportions, Whenever the same two elements combine to form more than one compound, the various masses of an individual element that combine with the same mass of the other elements exist in the ratio of small whole numbers.
Example - Consider carbon and oxygen atoms. Carbon and oxygen atoms combine to give two different types of products - Carbon monoxide and carbon dioxide. In carbon monoxide, the amount of oxygen present for one carbon atom i.e. 12.0grams is 16.0 grams. In carbon dioxide, the amount of oxygen present for one carbon atom 12.0 grams is 32.0 grams. The ratio of the amount of carbon present in carbon monoxide to the amount of carbon present in carbon dioxide is 32:16 or 2:1.
Gay Lussac’s proposed the law of gaseous volumes in 1808.
According to Gay Lussac’s law of gaseous volumes, the ratio of the volumes of all gaseous reactants and products can be represented in small whole numbers. When gases react at a particular pressure and temperature, the ratio of volumes of reactants and products can easily be expressed in small whole numbers.
Example - The combination of hydrogen gas and chlorine gas is governed by Gay Lussac’s law of gaseous volumes.
H2 + Cl2 → 2 HCl
In this example, one volume of Hydrogen gas combines with one volume of chlorine gas to produce 2 volumes of HCl gas. The ratio of the volume of hydrogen gas, chlorine gas, and HCl is 1:1:2.
Avagadro proposed the fifth law of chemical combination in 1811.
According to Avagadro’s law of chemical combination, at a given constant temperature and pressure, the volume of gaseous molecules is directly proportional to the total number of moles. Avogadro’s law is expressed as follows.
V ∝ n
Where V is the volume of gaseous molecules,
And n is the total number of moles of the gas.
V = k × n
Where k is the proportionality constant.
Where V1 is the volume and n1 is the number of moles of one gas. And V2 is the volume and n2 is the number of moles of another gas.
Example - Blowing of helium gas into a balloon. As the total number of moles of helium gas blown into the balloon increases, the overall volume of the balloon also increases.