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A reaction mixture is prepared containing 0.60 mol of aluminium and 1.20 mol of manganese dioxide. The mixture is heated until one of the reactants has been completely consumed according to the equation:
$2 Al + 3 {MnO}_{2} ⟶ 3 Mn + {Al}_{2} O_{3}$
What quantity of which reactant remains uncombined?

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0.20 mol Al

0.40 mol Al

0.30 mol MnO₂

0.60 mol MnO₂

answer is C.

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Detailed Solution

$LR \to Al$

$n_{{MnO}_{2}} left = 1.2 - \frac{0.0}{2} \times 3$

$= 0.3$

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