Answer :
Final answer:
To find the amount of Iron needed to react completely with 25.6 g of Oxygen to form iron(III) oxide (Fe2O3), we first convert the mass of Oxygen to moles. Then, using the stoichiometric ratio from the balanced chemical equation, we find the amount of Iron needed. However, none of the options given match the correct calculation result.
Explanation:
The subject matter is a stoichiometry problem in Chemistry. The formula Fe2O3 indicates the composition of iron(III) oxide, which consists of 2 atoms of Iron and 3 atoms of Oxygen. First, we need to convert the given weight of Oxygen into moles by using the molar mass of Oxygen. Then, we calculate the amount of Iron needed by using the stoichiometric ratio from the balanced chemical equation.
The molar mass of O is 16.00 g/mol, and we know from the formula Fe2O3 that 3 moles of O combines with 2 moles of Fe. Therefore, moles of O in 25.6 g are 25.6g / 16.00g/mol = 1.60 moles. Since 3 moles of O combines with 2 moles of Fe, the moles of Fe needed are 2/3 * 1.60 moles = 1.067 moles.
Since the molar mass of Fe is 55.85 g/mol, the mass of Fe needed is 55.85g/mol * 1.067 moles = 59.86g ≈ 60g. So none of the available options are correct.
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