Question

Use the law of constant composition to complete the following table summarizing the amounts of iron and chlorine produced upon the decomposition of the sample of iron(III) chloride. Mass FeCl3 Mass Fe Mass Cl Sample A3.785 g1.302 g2.483 g Sample B1.475 g _____ _____

Answer 1

So your question ask to complete the table in your problem using the law of constant composition and the table summarize the amount of iron and chlorine produced upon the decomposition of the sample iron and the data that would complete the table is FeCi3(162.2), Fe(0.508), Cl(0,967)

Answer 2

Answer : The mass of Fe and Cl in sample B is 3.341 g and 6.371 g respectively.

Explanation :

Law of definite proportion : It is defined as a given compound always contains exactly the same proportion of elements by weight.

The balanced chemical reaction will be,

$2FeCl_3\rightarrow 2Fe+3Cl_2$

First we have to calculate the ratio of mass of $FeCl_3$.

$\text{Ratio}=\frac{\text{Mass of }FeCl_3 \text{in sample A}}{\text{Mass of }FeCl_3 \text{in sample B}}$

$\text{Ratio}=\frac{3.785g}{1.475g}=2.566$

Now we have to calculate the mass of Fe and Cl in sample B.

$\text{Mass of Cl in sample B}=2.566\times \text{Mass of Cl in sample A}$

$\text{Mass of Cl in sample B}=2.566\times 2.483g=6.371g$

and,

$\text{Mass of Fe in sample B}=2.566\times \text{Mass of Fe in sample A}$

$\text{Mass of Fe in sample B}=2.566\times 1.302g=3.341g$

Therefore, the mass of Fe and Cl in sample B is 3.341 g and 6.371 g respectively.