Chemistry atomic structure

Question

An acidified solution of the salt KC1Ox (x = 1, 2 or 3) will oxidise Fe2(aq) to Fe3+(aq) quantitatively, the chlorine being reduced to Cl-(aq). When 0.150 g of the salt KClOx was reacted with 0.500 mol dm-3 Fe2+(aq) in the presence of H+ (aq), 11.3 cm3 of Fe2+(aq) was needed for complete reaction. Calculate the value of x and construct an equation for the reaction between Fe2+(aq) and acidified KCIOx

Answer 1

Possibilities would include

2Fe²⁺ + KClO + 2H⁺ ==> 2Fe³⁺ + KCl + H₂O

4Fe²⁺ + KClO₂ + 4H⁺ → 4Fe³⁺ + KCl + 2H₂O

6Fe²⁺ + KClO₃ + 6H⁺ → 6Fe³⁺ + KCl + 3H₂O

(0.500 mol dm^-3 Fe²⁺) x (0.0113 dm^3) = 0.00565 mol Fe²⁺

Looking at the 3 possibilities above, we have...

(0.00565 mol Fe²⁺) x (1 mol KClO / 2 molFe²⁺) x (90.6 g KClO/mol) = 0.256 g KClO

(0.00565 mol Fe²⁺) x (1 mol KClO₂ / 4 mol Fe²⁺) x (106.6 g KClO₂/mol) = 0.151 g KClO₂

(0.00565 mol Fe²⁺) x (1 mol KClO₃ / 6 mol Fe²⁺) x (122.5 g KClO₃/mol) = 0.115 g KClO₃

From these calculations, the second choice gives a mass equivalent to one given in the problem.

The salt would be KClO2 where x = 2

The equation would be 4Fe²⁺ + ClO₂^- + 4H⁺ ==> 4Fe³⁺ + Cl^- + 2H₂O