Question

In the reaction of iron and chlorine, what mass of iron is needed to prepare 11.86 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

The iron cation in the product is 1s22s22p63s23p63d6 means it is present as Fe2+

the product is FeCl2

Balanced Equation is

Fe + Cl2 >>> FeCl2

Now calculate the mole of FeCl2 in e 11.86g of FeCl2 :

11.86g of FeCl2 / 126.751 g/mol = 0.093 molFeCl2

Now number of moles of Fe from reaction:

0.093 molFeCl2 x 1 mol Fe / 1 mol FeCl2 = 0.093 molFe

Then calculate the mass of Fe in 0.093 molFe :

0.093 molFe x molar mass Fe =0.093 molFe x 55.845 g/mol = 5.19 g Fe