Question

5.58 gram iron reacted with 3.21 g sulfur. how many grams of iron sulfide were produced?

Answer 1

Answer:

8.79 gram

Explanation:

because 5.58 gram +3.21 gram

Answer 2

Concept:

Two reactants are combined into one product in a combination reaction. A synthesis reaction is another name for a combination reaction. The general form of the reaction is as follows: X + Y → XY.

Given:

Mass of iron = 5.58 g

Mass of sulfur = 3.21 g

Find:

5.58 gram iron reacted with 3.21 g sulfur. how many grams of iron sulfide was produced?

Solution:

Fe + S → FeS is the reaction's equation.

The two elements combine to generate iron(II) sulfide, or FeS, in a 1:1 molar ratio.

Iron's molar mass is 55.85 g/mol.

Sulfur's molar mass is 32.06 g/mol.

It is evident that only 32 g of sulfur may be combined with 55.85 g of iron. Since fewer than 7 g of sulfur will mix with 7 g of iron, iron serves as the limiting reagent in this reaction.

FeS has a molecular mass of 87.91 g/mol (55.85 + 32.06).

FeS produced from 55.85 g of iron equals 87.91 g.

FeS to be extracted from 7 g of iron =  $\frac{87.91 * 7}{55.85}$  = 11.02 g

Hence, when 5.58 grams of iron reacted with 3.21 g sulfur then 11.02 grams of iron sulfide was produced.

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