How much heat (in kJ) is evolved when 2.7 g of aluminium reacts with a stoichiometric amount of $Fe_{2}O_{3}$? $2Al_{2} + Fe_{2}O_{3} \rightarrow 2Fe + Al_{2}O_{3};\ \mathrm{\Delta}H^{o} = - 852\ kJ$

Question

Dr. Abubacker · Accepted Answer

(c)
$2Al + Fe_{2}O_{3} ightarrow 2Fe + Al_{2}O_{3};\mathrm{\Delta}H{^\circ} = - 852$ kJ
$\because 2$ mol Al (=54 g) evolved heat $= - 852$ kJ
$	herefore 2.7\ g$Al will evolve heat $= - \frac{852 	imes 2.7}{54}$
$= - 42.6$ kJ

Q. How much heat (in kJ) is evolved when 2.7 g of aluminium reacts with a stoichiometric amount of $Fe_{2}O_{3}$? $2Al_{2} + Fe_{2}O_{3} \rightarrow 2Fe + Al_{2}O_{3};\ \mathrm{\Delta}H^{o} = - 852\ kJ$

Explanation

Reviewed by Dr. Abubacker

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