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That depends on the oxidation state of the Fe.

Fe(II) or Fe(III)

Fe + Cl2 --> FeCl2 Fe(II)

Answer: 4.4 mol chlorine. The iron(II)chloride is normally prepared using hydrochloric acid rather than chlorine.

Fe + 1.5 Cl2 --> FeCl3

Answer: 6.6 mol

The iron(III)chloride is could be prepared using hot granulated iron in chlorine.

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If 6.0g of iron reacted with 6.0g of chlorine what is the maximum number of moles of iron-II chloride that can be produced?

The molar mass of FeCl2 is calculated as follows: Fe: 55.85 g/mol Cl: 35.45 g/mol FeCl2: 55.85 + 2(35.45) = 126.75 g/mol The number of moles of FeCl2 that can be produced is determined by the limiting reactant, which in this case is iron. Therefore, first calculate the number of moles of iron using its molar mass and then use the stoichiometry of the reaction to determine the maximum number of moles of FeCl2 that can be formed.


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