Part C. The elements X and Y combine in different ratios to form four different types of compounds: XY, XY2, XY3, and XY4. Consider that there is enough of each compound to contain 2 g of X. In XY the mass of X is 2 g and the mass of Y is 4 g. Arrange the following ratios in order of their increasing value.
Rank from highest to lowest ratio. To rank items as equivalent, overlap them.
The law of multiple proportions predates the concept of a mole or molar mass. Thus, scientists like John Dalton could only determine the relative amounts of each type of atom in a formula, and not the exact formula. For example, Dalton could determine that there were two carbon-oxygen compounds, one with twice as much oxygen as the other, but he could not know for sure what their formulas were. However, he could determine that the mass ratio of the elements in one compound was related to the mass ratio of elements in the other compound by a small whole number.
If two elements A and B combine to form two compounds AB and AB2 then the ratio of the mass of B to A in AB2 and the mass of B to A in AB will be a simple whole number.
When carbon reacts with a small amount of oxygen, the principle product formed is carbon monoxide (CO). When the oxidation occurs in a higher concentration of oxygen, the principle product formed is carbon dioxide (CO2). The mass ratio of oxygen to carbon in carbon dioxide (CO2) is twice the mass ratio of oxygen to carbon in carbon monoxide (CO).
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