Final answer:
The question involves calculation of heat released in a stoichiometry problem with a given chemical reaction. The limiting reactant is found to be Fe and by using the balanced chemical equation and the heat per mole of the reaction, the heat release for the given amount of reactants is found out to be approximately 74.6 kJ.
Step-by-step explanation:
The question is about stoichiometry and thermochemistry, specifically it is asking to calculate the amount of heat released when certain amounts of iron (Fe) and oxygen (O2) react according to the balanced chemical equation given.
We first need to find the moles of reactants involved. The molar mass of Fe is about 55.845 g/mol and of O2 it is about 32.00 g/mol.
So, Moles of Fe = mass / molar mass = 10 / 55.845 ≈ 0.179 moles. Similarly for O2,
Moles = mass / molar mass = 2/32 = 0.0625 moles.
According to the balanced chemical reaction, 4 moles of Fe react with 3 moles of O2 to release 1652 kJ of heat.
If 0.179 moles of Fe is available, it would require 0.179 * (3/4) ≈ 0.134 moles of O2. Since we have more than this amount available (0.0625), Fe is the limiting reagent.
From the balanced chemical equation, 1652 kJ of heat is released by the reaction of 4 moles of Fe. Therefore, by unitary method, the heat released by the reaction of 0.179 moles of Fe would be 1652 * 0.179 / 4 ≈ 74.6 kJ
The reaction thus releases about 74.6 kJ of heat when 10.0 grams of Fe and 2.00 grams of O2 are reacted.
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