o Assume two molecules of CO that is carbon monoxide and CO2 that is carbon dioxide
o CO contains 12 grams of carbon and 16 grams of oxygen
o CO2 contains 12 gram of carbon plus 32 grams of oxygen
o The ratio of mass of oxygen in each of the two compounds is expressed in the ratio 16 :32 which is equal to 1: 2
o Therefore, the law of multiple proportions is proved here.
o Another example of law of multiple proportions includes; Hydrogen and oxygen combine to form two compounds of H2O and one compound of hydrogen peroxide.
o Thus, the ratio of different weights of oxygen is 16 and 32 combining with a fixed weight of two hydrogen thus,16 I; 32 that is 1; 2 which is a simple whole number ratio.
o Therefore, Law of multiple proportions is proved here.
o Nitrogen reacts with oxygen to form numerous nitrogen oxides under various reaction conditions.
o Some of them include; nitrogen monoxide (NO), nitrogen dioxide (NO2), dinitrogen trioxide (N2O3), and dinitrogen pentoxide (N2O5).
o The amount of nitrogen taken is 14 g.
o When take the ratio of the amounts of oxygen that is required each reaction, thus the ratios obtained are 8:16:24:32:40 or 1:2:3:4:5.
o Thus, the ratio obtained is in small whole numbers and the given law of multiple proportions is also valid for more than two reactions.