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114. Match the columns
Column-1
Column-1
(Laws of chemical
(Scientist)
combinations)
(A) Law of definito
(p) Antoine Lavoisier
proportions
(B) Law of multiple
(9) Gay Lussac
proportions
(0) Law of conservation (0) Dalton
of mass
(D) Law of gaseous
(s) Joseph Proust
volumes
A-(s), B-(), C (p). D -(9)
(b) A --(p), B-(T), C-(S), D-(9)
(c) A-(1), B -(p), C-(s), D-(9)
(d) A-(9), B-(s), C-(!), D-(p)
on
ng
ts.
Answers
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 the 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 per cent 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 a simple ratio by volume given that all the gases are at the same temperature and pressure. This law can be considered as another form of the 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 the 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 the same conditions of temperature and pressure, an equal volume of all the gases contains an 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 the same temperature and pressure.
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