Question Solved1 Answer I do not want to explain by writing, calculations help me to understant better. The thermite reaction involves aluminum and iron(III) oxide 2Al(s) +Fe2O3(s) -Al2O3(s)+2Fe(1) This reaction is highly exothermic and the liquid iron formed is used to weld metals. > Calculate the heat released in kilojoules per gram of Al reacted with Fe2O3. The AH in kJ/ mol for Fe(/) is 12.40, Al2O3 -1669.8, and Fe203 - 822.2. The thermite reaction involves aluminum and iron(III) oxide 2Al(s) +Fe2O3(s) -Al2O3(s)+2Fe(1) This reaction is highly exothermic and the liquid iron formed is used to weld metals. > Calculate the heat released in kilojoules per gram of Al reacted with Fe2O3. The AH in kJ/ mol for Fe(/) is 12.40, Al2O3 -1669.8, and Fe203 - 822.2.

NN2XMT The Asker · Chemistry

I do not want to explain by writing, calculations help me to understant better.

Transcribed Image Text: The thermite reaction involves aluminum and iron(III) oxide 2Al(s) +Fe2O3(s) -Al2O3(s)+2Fe(1) This reaction is highly exothermic and the liquid iron formed is used to weld metals. > Calculate the heat released in kilojoules per gram of Al reacted with Fe2O3. The AH in kJ/ mol for Fe(/) is 12.40, Al2O3 -1669.8, and Fe203 - 822.2. The thermite reaction involves aluminum and iron(III) oxide 2Al(s) +Fe2O3(s) -Al2O3(s)+2Fe(1) This reaction is highly exothermic and the liquid iron formed is used to weld metals. > Calculate the heat released in kilojoules per gram of Al reacted with Fe2O3. The AH in kJ/ mol for Fe(/) is 12.40, Al2O3 -1669.8, and Fe203 - 822.2.
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Transcribed Image Text: The thermite reaction involves aluminum and iron(III) oxide 2Al(s) +Fe2O3(s) -Al2O3(s)+2Fe(1) This reaction is highly exothermic and the liquid iron formed is used to weld metals. > Calculate the heat released in kilojoules per gram of Al reacted with Fe2O3. The AH in kJ/ mol for Fe(/) is 12.40, Al2O3 -1669.8, and Fe203 - 822.2. The thermite reaction involves aluminum and iron(III) oxide 2Al(s) +Fe2O3(s) -Al2O3(s)+2Fe(1) This reaction is highly exothermic and the liquid iron formed is used to weld metals. > Calculate the heat released in kilojoules per gram of Al reacted with Fe2O3. The AH in kJ/ mol for Fe(/) is 12.40, Al2O3 -1669.8, and Fe203 - 822.2.
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Given the reaction here: -QAl(s)+Fe_(2)O_(3)(s)rarrAl_(2)O_(3)(s)+2Fe(l)DeltaH_(f)^(@)= Heat of formation of standard conditions. So,{:[(AH_(1)^(@))_(Al)=0kJ.],[(DeltaH_(f)^(@))_(Fe_(2)O_(3))=-822.2kJ//mol.],[(AH_(f)^(@))_(Al_(2)O_(3))=-1669.8kJ/ ... See the full answer