A metal X forms two different chlorides . If 12.7g of chloride A an 16.3g of chloride B contain 71g and figures agree with the law of multiple proportion .
Write the formulae
"contains 71 g of what?"
Ametal X forms two different chlorides . If 12.7g of chloride A an 16.3g of chloride B 71g and 10.87g of chloride respectively, show that the figures agree with the law of multiple proportion.
Write the formulae
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To determine the formulae of the chlorides, we must examine the relationship between the masses of the metal (X) and the masses of chlorine (Cl) in each chloride. From the information given, we have:
Mass of Chloride A (ClA) = 12.7g
Mass of Chloride B (ClB) = 16.3g
Next, we compare the ratios of the masses of the metal (X) to the masses of chlorine (Cl) in both chlorides.
For Chloride A:
Mass of X = Total Mass of Chloride A - Mass of Chlorine in Chloride A
= 12.7g - 71g (as given in the information)
= -58.3g
(Note: We have a negative mass here but it's just an arbitrary label. What is important is the ratio between X and Cl.)
For Chloride B:
Mass of X = Total Mass of Chloride B - Mass of Chlorine in Chloride B
= 16.3g - 71g (as given in the information)
= -54.7g
Since both chlorides are formed from the same metal X, the ratio of X to Cl should be the same in both cases, given the law of multiple proportions.
To find the simplest whole number ratio between X and Cl, we can calculate the ratio between the masses of X for both chlorides:
Ratio of X (ClA) to X (ClB) = Mass of X (ClA) / Mass of X (ClB)
= -58.3g / -54.7g
= 1.066
Since the ratio is close to 1, we can consider it as approximately 1:1. Therefore, the formula for Chloride A is XCl, and the formula for Chloride B is XCl.
Note: In a more complex example, we may need to use the concept of molar mass, atomic mass, and convert the masses into moles before determining the simplest whole number ratio. However, in this case, the given masses directly help us find the formulae.