How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3 (s) + 2 Al (s) → Al2O3 (s) + 2 Fe (s) ΔH°rxn = - 852 kJ

Question

Carley Randolph

Physics

20 April, 15:36

How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3 (s) + 2 Al (s) → Al2O3 (s) + 2 Fe (s) ΔH°rxn = - 852 kJ

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Jeramiah Mckenzie · Answer 1

From the reaction, we see that for every 2 moles of Al reacted, 852 kJ of energy is released. So convert the mass given to moles:

moles Al = 48.7 g / (26.98 g/mol)

moles Al = 1.805 mol

So the energy evolved is:

Energy = - 852 kJ / 2 mol * 1.805 mol

Energy = - 769 kJ