Using the stoichiometry of the reaction, we can obtain the molar mass of the complex as 276 g/mol. The number of moles iron II as 0.00181 moles and the mass of iron II as 0.1 g.
<h3>Redox reaction</h3>
A redox reaction is one in which there is loss or gain of electrons. The equation of the reaction is 5Fe2+ + MnO4- + 8H+ - - > 5Fe2+ + Mn2+ +4H2O
Number of moles of permanganate = 0.0200 mol. dm3 * 18.10cm3/1000 L
= 0.000362 moles
If 5 moles of iron II reacted with 1 mole of permanganate
x moles of iron II reacts with 0.000362 moles of permanganate
x = 5 moles * 0.000362 moles/ 1 mole
= 0.00181 moles of iron II
Recall that;
Number of moles = mass/molar mass
Molar mass of iron II = 56 g/mol
0.00181 moles = x/56 g/mol
x = 0.00181 moles * 56 g/mol = 0.1 g
If 1 mole of the complex contains 1 mole of iron then;
0.00181 moles = 500 * 10^-3/MM
MM= 500 * 10^-3/0.00181 moles
MM = 276 g/mol
Learn more about stoichiometry: brainly.com/question/9743981
