A Metal X forms two different chloride. If 12.7g of chloride A and 16.3g of chloride B contains 7.1g and 10.7g of chlorine respectively, show that the figure agree with the law of multiple proportion. Write their formulae
To determine if the figures agree with the law of multiple proportion, we need to compare the ratio of the masses of chlorine in each chloride.
First, let's calculate the ratio of chlorine in chloride A:
Mass of chlorine in chloride A = 7.1g
Mass of chloride A = 12.7g
Ratio = Mass of chlorine/Mass of chloride = 7.1g/12.7g
Now, let's calculate the ratio of chlorine in chloride B:
Mass of chlorine in chloride B = 10.7g
Mass of chloride B = 16.3g
Ratio = Mass of chlorine/Mass of chloride = 10.7g/16.3g
Now, let's simplify the ratios:
Ratio for chloride A = 7.1g/12.7g ≈ 0.559
Ratio for chloride B = 10.7g/16.3g ≈ 0.656
These ratios represent the ratio of chlorine to chloride in each compound.
To determine if the figures agree with the law of multiple proportion, we need to see if the ratios can be expressed as simple whole number ratios.
Dividing the ratio for chloride B by the ratio for chloride A:
(10.7g/16.3g) / (7.1g/12.7g) ≈ 1.172 / 0.559 ≈ 2.096
The result is not a simple whole number ratio, which indicates that the figures do not strictly follow the law of multiple proportions.
Now, let's write their formulae:
The formula for chloride A can be represented as MXCl2, where M is the metal.
The formula for chloride B can be represented as MXCl3, where M is the same metal.
Please note that this calculation assumes that all the chlorine is present in the chlorides and that there are no other elements involved in the compounds.