The following thermochemical equation is for the reaction of Fe with Cl2 to form FeCl3.
2Fe+3Cl2 -> 2FeCl3 ΔH=-799kj
How many grams of Fe would have to react to produce 100 kJ of energy?
________grams
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To find the grams of Fe that would react to produce 100 kJ of energy, we need to use the equation ΔH = n * ΔHrxn, where n is the number of moles of reacting species and ΔHrxn is the enthalpy change for the reaction.
In this case, we have ΔH = -799 kJ and we want to find n. Rearranging the equation, we have n = ΔH / ΔHrxn.
n = 100 kJ / (-799 kJ) = -0.125
Since moles cannot be negative, we discard the negative sign.
Now, we can use the balanced equation to determine the stoichiometry between Fe and FeCl3.
According to the equation, 2 moles of Fe react to produce 2 moles of FeCl3, so the stoichiometric ratio is 2:2.
Therefore, if n = 1 mole of FeCl3, then n = 0.5 moles of Fe.
The molar mass of Fe is 55.85 g/mol.
Therefore, the number of grams of Fe that would react to produce 100 kJ of energy is:
Grams of Fe = n * molar mass = 0.5 moles * 55.85 g/mol = 27.93 grams.
Therefore, 27.93 grams of Fe would have to react to produce 100 kJ of energy.
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