se the information provided to determine ΔH°rxn for the following reaction:
ΔH°f (kJ/mol) 3 Fe2O3(s) + CO(g) → 2 Fe3O4(s) + CO2(g) ΔH°rxn = ?
Fe2O3(s) -824
Fe3O4(s) -1118
CO(g) -111
CO2(g) -394
See your other post above.
To determine ΔH°rxn for the given reaction:
1. Write down the balanced equation for the reaction:
3 Fe2O3(s) + CO(g) → 2 Fe3O4(s) + CO2(g)
2. Look up the standard enthalpy of formation (ΔH°f) values for each compound involved in the reaction. The ΔH°f values provided are:
Fe2O3(s): -824 kJ/mol
Fe3O4(s): -1118 kJ/mol
CO(g): -111 kJ/mol
CO2(g): -394 kJ/mol
3. Determine the change in enthalpy (ΔH°rxn) by using the sum of the products minus the sum of the reactants:
ΔH°rxn = (2 × ΔH°f of Fe3O4) + (ΔH°f of CO2) - (3 × ΔH°f of Fe2O3) - (ΔH°f of CO)
Substituting the ΔH°f values into the equation:
ΔH°rxn = (2 × -1118) + (-394) - (3 × -824) - (-111)
Simplifying the equation:
ΔH°rxn = -2236 - 394 + 2472 + 111
ΔH°rxn = -303 kJ/mol
Therefore, ΔH°rxn for the given reaction is -303 kJ/mol.