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The empirical formulas of the two oxides are CO and [tex]CO_2[/tex] respectively. Thus, the figures illustrate the law of multiple proportions.
The law of multiple proportions states that when two elements form more than one compound, the ratios of the masses of the second element which combine with a fixed mass of the first element will always be ratios of small whole numbers.
Now, let's see if the figures quoted in the problem obey this law:
The first oxide:
C = 42.9
O = 100-42.9
= 57.1
The equivalent mole of each atom would be:
C = 42.9/12
= 3.56
O = 57.1/16
= 3.56
Thus, the empirical formula of the first oxide is CO.
The second oxide:
C = 27.3
O = 100 - 27.3
= 72.7
The equivalent mole of each atom will be:
C = 27.3/12
= 2.27
O = 72.7/16
= 4.54
Dividing the moles by the smallest mole
C = 2.27/2.27
= 1
O = 4.54/2.27
= 2
Thus, the empirical formula of the second oxide is [tex]CO_2[/tex].
In other words, the figures quoted obeys the law of multiple proportions.
More on the law of multiple proportions can be found here: https://brainly.com/question/28458716
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