Use the given ΔH°f data to calculate the ΔH°rxn for the "thermite reaction" below:

{Al2O3(s), ΔH°f = –1669.8 kJ/mol; Fe(l), ΔH°f = 12.40 kJ/mol; Fe2O3(s), ΔH°f = –822.2 kJ/mol}

2Al(s) + Fe2O3(s) → Al2O3(s) + 2Fe(l) ΔH°rxn = ??

Question

Use the given ΔH°f  data to calculate the ΔH°rxn for the "thermite reaction" below:

{Al2O3(s), ΔH°f  = –1669.8 kJ/mol; Fe(l), ΔH°f  = 12.40 kJ/mol; Fe2O3(s), ΔH°f  = –822.2 kJ/mol}

2Al(s)  +  Fe2O3(s)  →  Al2O3(s)  +  2Fe(l)               ΔH°rxn = ??

aaronq · Answer

do you know Hess's law?   $H^o_{(rxn)}=\Sigma H^o_{f~(products)}-\Sigma H^o_{f~(reactants)}$