Q.Explain the law of multiple proportion with examples.
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Start your 14-day free trial to unlock the full solution →Law of multiple proportions (Dalton): when two elements form two or more compounds, the different masses of one element that combine with a fixed mass of the other are in a simple whole-number ratio.
Statement: If two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in the ratio of small whole numbers.
Example 1 — Carbon and Oxygen:
Carbon combines with oxygen to form two compounds: carbon monoxide (CO) and carbon dioxide (CO2).
In CO, 12 g of carbon combines with 16 g of oxygen.
In CO2, 12 g of carbon combines with 32 g of oxygen.
For the same fixed mass of carbon (12 g), the masses of oxygen are 16 g and 32 g, which are in the ratio 16:32 = 1:2 — a simple whole-number ratio.
Example 2 — Nitrogen and Oxygen:
Nitrogen forms several oxides: N2O, NO, N2O3, NO2, N2O5.
For a fixed mass of nitrogen (28 g, i.e. 2 mol N), the masses of oxygen combining are 16 g, 32 g, 48 g, 64 g, and 80 g respectively — in the ratio 1:2:3:4:5, again simple whole numbers.
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