Answer:
Here's what I get.
Explanation:
The Law of Multiple Proportions states that when two elements A and B combine to form two or more compounds, the masses of B that combine with a given mass of A are in the ratios of small whole numbers.
That is, if one compound has a ratio r₁ and the other has a ratio r₂, the ratio of the ratios r is in small whole numbers.
1. Oxide A
Mass of O = 1 - 0.881 = 0.119 g
[tex]r_{1} = \dfrac{\text{mass of O}}{\text{mass of M}} = \dfrac{ 0.119}{0.881} = 0.1351[/tex]
2. Oxide B
Mass of O = 1 - 0.788 = 0.212 g
[tex]r_{2} = \dfrac{ 0.212}{0.788} = 0.2690[/tex]
3. Ratio of the ratios
[tex]r = \dfrac{r_{1}}{r_{2}} = \dfrac{ 0.1351}{0.2690} = \dfrac{1 }{1.992} \approx \dfrac{1}{2}\\\\\text{The relative amounts of O per gram of M in the two oxides are in the ratio $\large \boxed{\mathbf{\dfrac{1}{2}}}$}[/tex]
