Question:

How many grams of FeCl2 can be produced when 4.5 g of Fe reacts with 5.5 g of Cl2?

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How many grams of FeCl2 can be produced when 4.5 g of Fe reacts with 5.5 g of Cl2?

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  1. The maximum amount produced will be from the reaction of all of the limiting reagent.

    To work out which is the limiting reagent first work out the number of moles of each reactant started with use the equation.

    moles = mass / molecular weight

    molecular weight Fe = 55.85 g/mol

    moles Fe = 4.5 g / 55.85 g

    = 0.0806 moles of Fe

    molecular weight Cl2 = (2 x 35.45) = 70.9 g/mol

    moles Cl2 = 5.5 g / 70.9 g/mol

    = 0.0776 moles of Cl2

    The balanced equation for the reaction is

    Fe + Cl2 ------------> FeCl2

    This tells us that Fe and Cl2 react in a 1:1 ratio.

    Therefore the limiting reagent is Cl2 (0.0776 mol) and the Fe is in excess.

    Now, 1 mole of Cl2 reacts to give 1 mole of FeCl2. Therefore if you only have 0.0776 mole of Cl2 then the maximum FeCl2 you can produce is 0.0776 mol

    Mass of FeCl2 possible = mole x molecular weight

    molecular weight = 55.85 + (2 x 35.45) = 126.75 g/mol

    Therfore mass = 0.0776 mol x 126.75 g/mol

    = 9.84 g

    Therfore 9.84 g of FeCl2 is possible

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