Final answer:
To determine the heat of reaction (ΔHrxn) for the given reaction, we can use Hess's law. By breaking down the reaction into three steps and considering the enthalpy changes of each step, we can determine the overall enthalpy change of the reaction. In this case, the heat of reaction is -791.8 kJ/mol of Fe2O3.
Step-by-step explanation:
To determine the heat of reaction (ΔHrxn) for the given reaction, we can use Hess's law. According to Hess's law, the enthalpy change for a reaction can be calculated by considering the enthalpy changes of other related reactions. In this case, we can break down the reaction into three steps: the formation of 1 mol of solid aluminum oxide (Al2O3) and 2 mol of liquid iron, the conversion of 2 mol of liquid iron to 2 mol of solid iron, and the conversion of 2 mol of solid iron at high temperature to 2 mol of solid iron at room temperature.
The enthalpy changes for these reactions are given in the information provided. By summing up the enthalpy changes of these three reactions, we can determine the overall enthalpy change of the reaction we are interested in. In this case, ΔHrxn = -732.5 kJ/mol of Fe2O3 + (-13.8 kJ/mol of Fe) + (-45.5 kJ/mol of Fe) = -791.8 kJ/mol of Fe2O3.