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The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental iron, has been...

The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 

2Al(s) + Fe2O3(s) - 2Fe(s) + Al2O3(s)  AH=-850 kJ 


What mass of iron is formed when 725 kJ of heat are released?

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Answer #1

2 Al(s) +  Fe₂O₃ (s) ⇒ 2 Fe(s) + Al₂O₃(s) ΔHrxn = –850 kJ
as you see that negative sign show the reaction is exothermic but we have to take only magnitude for our answer.

from reaction, we see that 2 mole Al and 1 mole Fe₂O₃ gives 2 mole of iron in which 850KJ energy is released to the surrounding. So,
850 KJ energy released when 2 mole of iron is formed.
1 KJ energy released when 2/850 mole of iron is formed.
725 KJ energy released = 2/850 *725 mole of iron formed.
= 1.7 mole iron
molar mass of Fe is 55.6 g/mol

1 mole of iron = 55.6 g of iron
So, 1.7 mole of iron = 55.6 g * 1.7
= 94.85 g of iron is formed.

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