State avayardo's law of chemical combination with example.
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Hey mate
Here is Ur ans
This law states that equal volume of all gases under the same condition of temperature and pressure contain equal no of molecules.
V is directly proportional to n
Hope it helps u
ße ßrainly.
.....
.,✌️✌️❤️❤️❤️❤️
Here is Ur ans
This law states that equal volume of all gases under the same condition of temperature and pressure contain equal no of molecules.
V is directly proportional to n
Hope it helps u
ße ßrainly.
.....
.,✌️✌️❤️❤️❤️❤️
dundu002:
can we give an example like that
can i do later i have to go
but iWill do
kk
in which school are u stdig
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There are basically two laws of chemical combination -Law of conservation of mass andLaw of constant proportion.
The law of conservation of mass
states that the mass of a closed system will remain constant in a chemical reaction. In other words, mass can neither be created nor destroyed in a chemical reaction. This law was first formulated by Antoine Laurent Lavoisier in 1789.
For example, 100 g of mercuric oxide, when heated in a closed test tube, decomposes to produce 92.6 g of mercury and 7.4 g of oxygen gas.
2 HgO (s) → 2Hg (l) + O2(g).
Total mass of the reactant = 100 g
Total mass of the products = 92.6 + 7.4 g =100 g
Hence, during the decomposition reaction,matter is neither created nor destroyed. Here, matter is made up of tiny mercuric (Hg) and oxygen (O) atoms. The given reaction shows that atoms can neither be created nor destroyed in chemical reactions.
According to thelaw of constant proportion, a chemical substance always contains the same elements in a fixed proportion by mass, irrespective of its source. The law of constant proportion is also known as the law of definite proportion. This law, which was introduced by Proust, stated that ‘in a compound, the elements are always present in definite proportions by mass’.
For example, pure water obtained from anysource (well, river, lake, or sea) and from any country (India, Russia, America, etc.) will always contain two hydrogen atoms and one oxygen atom. Hydrogen and oxygen respectively combine together in the ratio of 1:8 by mass to form water. The ratio by the number of atoms for water will always be H : O = 2 : 1. Thus, 18 g of water contains 2 g of hydrogen and 16 g of oxygen.Similarly, in ammonia, nitrogen makes up 14/17 of the mass of ammonia while hydrogen makes up the remaining 3/17 of the mass. Irrespective of the source from which ammonia is obtained, itwill always contain nitrogen and hydrogen in the ratio of 14: 3 by mass. Thus, 17 g of ammonia contains 14 g of nitrogen and 3 gof hydrogen, and 34 g of ammonia contains 28 g of nitrogen and 6 g of hydrogen.
The law of conservation of mass
states that the mass of a closed system will remain constant in a chemical reaction. In other words, mass can neither be created nor destroyed in a chemical reaction. This law was first formulated by Antoine Laurent Lavoisier in 1789.
For example, 100 g of mercuric oxide, when heated in a closed test tube, decomposes to produce 92.6 g of mercury and 7.4 g of oxygen gas.
2 HgO (s) → 2Hg (l) + O2(g).
Total mass of the reactant = 100 g
Total mass of the products = 92.6 + 7.4 g =100 g
Hence, during the decomposition reaction,matter is neither created nor destroyed. Here, matter is made up of tiny mercuric (Hg) and oxygen (O) atoms. The given reaction shows that atoms can neither be created nor destroyed in chemical reactions.
According to thelaw of constant proportion, a chemical substance always contains the same elements in a fixed proportion by mass, irrespective of its source. The law of constant proportion is also known as the law of definite proportion. This law, which was introduced by Proust, stated that ‘in a compound, the elements are always present in definite proportions by mass’.
For example, pure water obtained from anysource (well, river, lake, or sea) and from any country (India, Russia, America, etc.) will always contain two hydrogen atoms and one oxygen atom. Hydrogen and oxygen respectively combine together in the ratio of 1:8 by mass to form water. The ratio by the number of atoms for water will always be H : O = 2 : 1. Thus, 18 g of water contains 2 g of hydrogen and 16 g of oxygen.Similarly, in ammonia, nitrogen makes up 14/17 of the mass of ammonia while hydrogen makes up the remaining 3/17 of the mass. Irrespective of the source from which ammonia is obtained, itwill always contain nitrogen and hydrogen in the ratio of 14: 3 by mass. Thus, 17 g of ammonia contains 14 g of nitrogen and 3 gof hydrogen, and 34 g of ammonia contains 28 g of nitrogen and 6 g of hydrogen.
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