In compound A, 1.00 g nitrogen unites with 0.57 g oxygen. In compound B, 2.00 g nitrogen combines with 2.24 g oxygen. In compound C, 3.00 g nitrogen combines with 5.11 g oxygen. These results obey the following law

Question

In compound A, 1.00 g nitrogen unites with 0.57 g oxygen. In compound B, 2.00 g nitrogen combines with 2.24 g oxygen. In compound C, 3.00 g nitrogen combines with 5.11 g oxygen. These results obey the following law (A) Law of constant proportion (B) Law of multiple proportion (C) Law of reciprocal proportion (D) Dalton’s law of partial pressure

Tardigrade Admin · Accepted Answer

Here, According to the question
Compound

A : 1.00 g N + 0.57 g O_{2}

Compound

B : 2.00 g N + 2.24 g O_{2}

Compound

C : 3.00 g N + 5.11 O_{2}

So If we fixed the amount of nitrogen

(1 g)

for all compound then,
Compound A:

1.00 g

of

N

combine with

0.57 g

of

O_{2}

Compound B :

2 g N

of

N

combine with

2.24 g

of

O_{2}

1 N = 1.12 g O_{2}

Compound C:

3 g N

combine with

5.11 O_{2}

1 g N = 1.70 g O_{2}

Thus,
Take in consideration the ratio of oxygen of all three compounds for the fixed amount of Nitrogen then we get
Ratio of oxygen

\approx 1 : 2 : 3

This ratio indicates the law of multiple proportion.

Q. In compound A,1.00g nitrogen unites with 0.57g oxygen. In compound B,2.00g nitrogen combines with 2.24g oxygen. In compound C,3.00g nitrogen combines with 5.11g oxygen. These results obey the following law

Law of constant proportion

Law of multiple proportion

Law of reciprocal proportion

Dalton’s law of partial pressure

Q. In compound $A, 1.00 g$ nitrogen unites with $0.57 g$ oxygen. In compound $B, 2.00 g$ nitrogen combines with $2.24 g$ oxygen. In compound $C, 3.00 g$ nitrogen combines with $5.11 g$ oxygen. These results obey the following law