Question

in the reaction of iron and chlorine, what mass of iron is needed to prepare 2 g of the iron chloride product if, under the conditions of the reaction, the electron configuration of the iron cation in the product is 1s22s22p63s23p63d6?

Answer 1

To prepare 2 g of iron chloride product, approximately 0.873 g of iron is needed.

Step-by-step explanation:

The molar mass of iron chloride (FeCl₂) is 126.75 g/mol. To find the mass of iron needed to prepare 2 g of FeCl₂, you can use the molar ratio from the balanced equation. The balanced equation for the reaction of iron and chlorine is:

2 Fe + 3 Cl₂ → 2 FeCl₂

From this equation, you can see that 2 moles of Fe react with 3 moles of Cl₂ to produce 2 moles of FeCl₂. Therefore, the ratio of Fe to FeCl₂ is 2:2. Using this ratio, you can set up a proportion to find the mass of Fe needed:

(mass of Fe) / (mass of FeCl₂) = (molar mass of Fe) / (molar mass of FeCl₂)

Plugging in the values, you get:

(mass of Fe) / 2 g = 55.85 g/mol / 126.75 g/mol

Solving for the mass of Fe:

mass of Fe = (2 g)(55.85 g/mol) / 126.75 g/mol ≈ 0.873 g