Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of the hydrogen that combines with 1.00g of each compound is 1.4 x 10^-1g, 2.4x10^-1 g and 2.40x10^-2 respectively. Show how these data illustrate the law of multiple proportions.

Question

Aldo Jennings

Chemistry

13 December, 15:20

Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of the hydrogen that combines with 1.00g of each compound is 1.4 x 10^-1g, 2.4x10^-1 g and 2.40x10^-2 respectively. Show how these data illustrate the law of multiple proportions.

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Rivas · Answer 1

The law of multiple proportions, states that when two elements combine to form more than one compound, the mass of one element, which combines with a fixed mass of the other element, will always be ratios of whole numbers. You divide each by the smallest, and you should get the right kind of ratio. We do as follows:

H in N2H4 = 1.4x10^-1

1.4x10^-1 / 2.4x10^-2 = 6

H in NH3 = 2.4x10^-1

2.4x10^-1 / 2.4x10^-2 = 10

H in HN3 = 2.4x10^-2

2.4x10^-2 / 2.4x10^-2 = 1

Jovanni Booth · Answer 2

Hello there.

Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of the hydrogen that combines with 1.00g of each compound is 1.4 x 10^-1g, 2.4x10^-1 g and 2.40x10^-2 respectively. Show how these data illustrate the law of multiple proportions.

H in HN3 = 2.4x10^-2

2.4x10^-2 / 2.4x10^-2 = 1