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In the reaction of aluminum and iron(III) oxide to form iron and aluminum oxide, ΔH is -850 kJ. How many grams of aluminum oxide are formed when 350 kJ of heat are released? 2 Al (s) + Fe2O3 (s) → 2 Fe (s) + Al2O3 (s) ΔH= -850 kJ

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Answer:

When 350 kJ are released there are formed 41,98 g of aluminium oxide.

Explanation:

For the reaction:

2Al (s) + Fe₂O₃ (s) → 2Fe (s) + Al₂O₃(s)

There are produced 850 kJ.

350 kJ of energy produced are when are formed:

350 kJ × [tex]\frac{1 mol Al_{2}O_{3}}{850 kJ}[/tex] = 0,412 moles of Aluminium oxide.

As molar mass of aluminium oxide is 101,96 g/mol. The grams in 0,412 moles of Al₂O₃ are:

0,412 moles Al_{2}O_{3} × [tex]\frac{101,96g}{1mol}[/tex] = 41,98 g

Thus, when 350 kJ are released there are formed 41,98 g of aluminium oxide.

I hope it helps!