Two oxides of lead were separately reduced to metallic lead by heating in a current of hydrogen and the following data obtained: (i) Mass of yellow oxide =3.45 g, Loss in mass during reduction =0.24 g (ii) Mass of brown oxide =1.227 g, Loss in mass during reduction =0.16 g Show that the above data illustrate the Law of Multiple Proportions.

Asked by Anvita Chaudhary | 12th Jan, 2014, 04:08: PM

Expert Answer:

Let us consider the mass of oxygen as 1 g.

Mass of lead obtained from yellow oxide = 3.45 g – 0.24 g = 3.21 g

Mass of oxygen = 0.24 g

The mass of lead that combines with 0.24 g of oxygen = 3.21 g

Therefore, mass of lead that combines with 1 g of oxygen = 3.21/ 0.24 = 13.4 g

Mass of lead obtained from brown oxide = 1.227 g – 0.16 g = 1.067

Mass of oxygen = 0.16g

The mass of lead that combines with 0.16 g of oxygen = 1.067 g

Therefore, mass of lead that combines with 1 g of oxygen = 1.067/ 0.16 = 6.66 g

Now, ratio of masses of lead which combines with a fixed mass of oxygen = 13.4 : 6.66

= 2 :1

Thus, masses of lead which combine with the fixed mass of oxygen are in the ratio of (2:1) i.e. small whole numbers.

Hence, the law of multiple proportions is illustrated.

Answered by Hanisha Vyas | 13th Jan, 2014, 07:47: PM

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