Which one of the following pairs of compounds illustrates the law of multiple proportions?

Which one of the following sets of compounds correctly illustrates the law of reciprocal proportions?

Hydrogen combines with oxygen to form $H_2O$ in which $16 \ g$ of oxygen combine with $2 \ g$ of hydrogen. Hydrogen also combines with carbon to form $CH_4$ in which $2 \ g$ of hydrogen combine with $6 \ g$ of carbon. If carbon and oxygen combine together then they will do so in the ratio of

$n_1 \ g$ of substance $X$ reacts with $n_2 \ g$ of substance $Y$ to form $m_1 \ g$ of substance $R$ and $m_2 \ g$ of substance $S$. The reaction is represented as $X + Y \rightarrow R + S$. What is the relationship between the mass of the reactants and the mass of the products?

$1.0 \ g$ of an oxide of $A$ contained $0.5 \ g$ of $A$. $4.0 \ g$ of another oxide of $A$ contained $1.6 \ g$ of $A$. The data indicate the law of:

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: