![]() ![]() Of course we just as easily could have illustrated the law by considering the mass of nitrogen that combines with one gram of oxygen it works both ways!.Note that just as the law of multiple proportions says, the weight of oxygen that combines with unit weight of nitrogen work out to small integers. Line is obtained by dividing the figures the previous line by the smallest O:N ratio in the line above, which is the one for N 2O.But someone who depends solely on experiment would work these out by finding the mass of O that combines with unit mass (1 g) of nitrogen. ![]() The numbers in Line are just the mass ratios of O:N, found by dividing the corresponding ratios in line 1.(These numbers were not known in the early days of Chemistry because atomic weights (i.e., molar masses) of most elements were not reliably known.) These ratios were calculated by simply taking the molar mass of each element, and multiplying by the number of atoms of that element per mole of the compound. ![]()
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