Question

How much energy is evolved during the formation of 102 g of Al2O3, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s), H°rxn = -852 kJ

Answer 1

The energy evolved during the formation of 102 g of Al2O3 is approximately -5817.5 kJ.

Step-by-step explanation:

According to the given equation Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) and the enthalpy change (ÄHrxn) of -852 kJ, we can calculate the energy evolved during the formation of 102 g of Al2O3.

To find the energy evolved for the formation of 1 mole of Al2O3, we divide the enthalpy change by the molar ratio of Al2O3 to Fe2O3, which is 1:1. Therefore, the energy evolved per mole of Al2O3 is -852 kJ/mol.

Next, we calculate the number of moles of Al2O3 formed from 102 g using its molar mass. Then, we multiply the moles of Al2O3 by the energy evolved per mole to find the total energy evolved.

By substituting the values, the energy evolved during the formation of 102 g of Al2O3 is approximately -5817.5 kJ.