Question

Q.23. Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of hydrogen that combines with 1.00 g of nitrogen for each compound is 1.44 x 10^-1g, 2.16 x 10^-1g, and 2.40 x 10^-2g, respectively. Show how these data illustrate the law of multiple proportions.

Short answer

Answer

The ratio of the mass of hydrogen that combines with 1.0 g of nitrogen is:

1.44 x 10^-1g:2.16 x 10^-1g:2.40 x 10^-2g

= 6:9:1

Which is in multiples, and it obeys the law of multiple proportions.

Step-by-step solution

Step-by-Step SolutionStep 1: Statement about the multiple proportions law

When there is a formation of serious compounds using two elements, the ratio of the mass of the second element will combine with 1 g of the first element and reduces to a whole number.

The compounds of nitrogen and hydrogen

The molecular formula of hydrazine is NH₂-NH₂

The molecular formula of ammonia is NH₃.

The molecular formula of hydrogen azide is N₃H .

The mass of hydrogen that combines with 1g of nitrogen in this compound is:

1.44 x 10^-1g, 2.16 x 10^-1g, and 2.40 x 10^-2g respectively.

Illustration of multiple proportion law using given data

The ratio of the mass of hydrogen that combines with 1.0 g of nitrogen is:

1.44 x 10^-1g:2.16 x 10^-1g:2.40 x 10^-2g

= 6:9:1

Which is in multiples, and it obeys the law of multiple proportions.