A metal x form different chlorides.If 12.7g of chloride A and 16.3g of chloride B contains 7.1g and 10.7g of chlorine respectively show that the figures agree with the law of multiple proportions. write their formular
To show that the figures agree with the law of multiple proportions, we need to determine the ratio of the masses of chlorine in chloride A and chloride B.
Let's assume that the formula of chloride A is AxCl and the formula of chloride B is BxCl.
Given:
Mass of chloride A = 12.7g
Mass of chlorine in chloride A = 7.1g
Therefore, the mass of metal X in chloride A = (Mass of chloride A) - (Mass of chlorine in chloride A)
Mass of metal X in chloride A = 12.7g - 7.1g = 5.6g
Similarly,
Given:
Mass of chloride B = 16.3g
Mass of chlorine in chloride B = 10.7g
Therefore, the mass of metal X in chloride B = (Mass of chloride B) - (Mass of chlorine in chloride B)
Mass of metal X in chloride B = 16.3g - 10.7g = 5.6g
Now, let's compare the ratio of the masses of metal X to chlorine in both compounds:
Ratio in chloride A = (Mass of metal X in chloride A) / (Mass of chlorine in chloride A)
Ratio in chloride A = 5.6g / 7.1g = 0.79
Ratio in chloride B = (Mass of metal X in chloride B) / (Mass of chlorine in chloride B)
Ratio in chloride B = 5.6g / 10.7g = 0.52
The ratio of the masses should be a simple whole number ratio for the law of multiple proportions to hold. Since the ratios in chloride A and chloride B do not match, it indicates that the assumption of the formulas AxCl and BxCl is incorrect.
Therefore, we cannot determine the formulas of chloride A and chloride B based on the given information.
To show that the figures agree with the Law of Multiple Proportions, we need to examine the ratio of the masses of chlorine in chloride A and chloride B.
The Law of Multiple Proportions states that when two elements form more than one compound, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers.
Let's calculate the ratio of chlorine mass in chloride A and chloride B:
Chlorine mass in chloride A = 7.1g
Chlorine mass in chloride B = 10.7g
Now, we divide the mass of chlorine in chloride B by the mass of chlorine in chloride A:
Ratio = (Chlorine mass in chloride B) / (Chlorine mass in chloride A) = 10.7g / 7.1g = 1.51
The ratio obtained is approximately 1.51.
To demonstrate the Law of Multiple Proportions, the ratio should be a simple whole number. In this case, the ratio is not a whole number. Hence, these figures do not perfectly adhere to the Law of Multiple Proportions.
However, we can determine the formulas for chloride A and chloride B based on the given information:
Let's assume the metal X has a fixed mass of "m" grams.
In chloride A:
Mass of chlorine = 7.1g
Mass of metal X = 12.7g - 7.1g = 5.6g
The ratio of chlorine to metal X is approximately 7.1g:5.6g, which simplifies to about 1.27:1. This ratio can be rounded to 1:1.
Therefore, the formula for chloride A is XCl.
In chloride B:
Mass of chlorine = 10.7g
Mass of metal X = 16.3g - 10.7g = 5.6g
Again, the ratio of chlorine to metal X is approximately 10.7g:5.6g, which simplifies to about 1.91:1. This ratio can be rounded to 2:1.
Therefore, the formula for chloride B is XCl2.
In conclusion, the formulas for chloride A and chloride B are XCl and XCl2, respectively.