Question

WHAT ARE THE 5 LAWS OF CHEMICAL COMBINATION . PLS EXPLAIN PROPERLY WITH EXAMPLES. ONLY VERIFIED ANSWERS✔✔ .... NO SPAMMING ❌❌​

Answer 1

☆Answer☆

1. Law of Conservation of Mass

In simple terms, this law states that matter can neither be created nor destroyed. In other words, the total mass, that is, the sum of mass of reacting mixture and the products formed remains  constant. Antoine Lavoisier gave this law in the year 1789 based on the data he obtained after carefully studying numerous combustion reactions.

2. Law of Definite Proportions

Joseph Proust, a French chemist stated that the proportion of elements by weight in a given compound will always remain exactly the same. In simple terms we can say that, irrespective of its source, origin or its quantity, the percent composition of elements by weight in a given compound will always remain the same.

3. Law of Multiple Proportions

This law states that if two elements combine to form more than one compound, the masses of these elements in the reaction are in the ratio of small whole numbers. This law was given by Dalton in the year 1803.

4.  Gay Lussac’s Law of Gaseous Volumes

In 1808, Gay Lussac gave this law based on his observations. This law states that when gases are produced or combine in a chemical reaction, they do so in simple ratio by volume given that all the gases are at same temperature and pressure. This law can be considered as another form of law of definite proportions. The only difference between these two laws of chemical combination is that Gay Lussac’s Law is stated with respect to volume while law of definite proportions is stated with respect to mass.

5. Avogadro’s Law

Avogadro proposed this law in the year 1811. It stated that under same conditions of temperature and pressure, equal volume of all the gases contain equal number of molecules. This implies that 2 litres of hydrogen will have the same number of molecules as 2 litres of oxygen given that both the gases are at same temperature and pressure.

The laws of chemical combination discussed above form the base for quantitative study of chemical reactions.

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Answer 2

Law of Chemical Combination

1) The law of conservation of mass:

• According to this law : "Matter can neither be created nor destroyed "
• This law was given by "Lavoisier
• Exception in nuclear reactions

Example : 2Mg +O2 →2MgO

Mass of Reactant = 2Mg+O2

= 2×24+ 32 =80

Mass of product =2×(24+16) =80

⇒Total Mass of Reactant=total of Reactant

2)The law of definate proportion:

• according to this law:" all pure samples of the same chemical compound contains the same elements combine in the same proportion by mass".
• This law given by "Proust "

Example :In H2O ratio weight of hydrogen to oxygen is 1:8

3) The law of Multiple Proportion:

• It states that " if two elements can combine to form more than one compound, the masses of one element that combines with a fixed mass of other elements ,are in the same ratio.
• Law Given by "Dalton".

Example :

Ratio of Masses of oxygen in H2O and H2O2 =16:32 =1:2

4)Avaogadro law :

• It states"equal volumes of all gases under similar condition temperature and pressure contain equal number of molecules".
• It provides a method to determine the molecular weight of gaseous elements .

Example :2H2(g) + O2(g)→2H2O(g)

⇒Ratio of no. of molecules =2:1:2

5)Gay Lussac law of gaseous Volumes :

• Law given by "Gay Lussac".
• It states that when gases combine or are produced in a chemical reaction ,they do so in a simple ratio by volume provided all gases are at same temperature and pressure.

Example : H2(g) +Cl2(g)→2HCl

⇒Ratio :1:1:2