$2 M g (s) + O_{2} (g) \to 2 M g O (s)$
If $0.243 g$ of magnesium is fully oxidized, what volume of oxygen will be used up? Assume STP conditions.

112 m L

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2443 m L

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448 m L

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0.486 m L

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Solution

The correct option is A $112 m L$
Given, $2 M g + O_{2} (g) \to 2 M g O$
At STP to burn $2 m o l e s$ of Magnesium we need $22.4 L i t r e s$ of Oxygen
$2 m o l e s$ of Magnesium $= 2 \times (24.3) = 48.6 g$
So, $48.6 g$ Magnesium $\to 22.4 L i t r e s$ of Oxygen is needed.
$0.243 g$ $\to (X)$
$\Rightarrow X = \frac{22.4 L \times 0.243}{48.6} = 0.112 L = 112 m L$

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