Problem: How much energy is evolved during the formation of 98.7 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)  ΔH°rxn = -852 kJ a) 1.51 x 103 kJ b) 241 kJ c) 482 kJ d) 4.20 x 103 kJ e) 753 kJ

FREE Expert Solution

We’re being asked to determine the heat (q) evolved by the reaction of 98.7 g Fe

The given reaction is:

Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)  ΔH°rxn = -852 kJ 


From the balanced equation, we can see that the given ΔH˚rxn (-852 kJ) corresponds to 2 mole of Fe


Recall that at constant pressure, heat is equivalent to enthalpy.


q(heat) = H(enthalpy)


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Problem Details

How much energy is evolved during the formation of 98.7 g of Fe, according to the reaction below? 

Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)  ΔH°rxn = -852 kJ 

a) 1.51 x 103 kJ 

b) 241 kJ 

c) 482 kJ 

d) 4.20 x 103 kJ 

e) 753 kJ


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