What weight of $A l$ will be completely oxidised by $44.8$ lit of oxygen at STP?

18

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37.8

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50.4

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72

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Solution

The correct option is D $72$ g

$4 A l + 3 O_{2} \to 2 A l_{2} O_{3}$

Ratio of moles $4$ $:$ $3$

$3 m o l e s$ oxygen oxidizes $4 m o l e s A l$

$2 m o l e s$ oxygen oxidizes $x m o l e s A l$

$x = \frac{2 \times 4}{3} = \frac{8}{3} = 2.66 m o l e s A l$

Weight of $2.66 m o l e s A l = 27 \times 2.66 = 71.82 g \approx 72 g$

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