The volume of oxygen at STP required to burn $2.4$ g of carbon completely is:

1.12

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8.96

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2.24

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4.48

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Solution

The correct option is C $8.96$ L
$C H_{4} + 2 O_{2} \to C O_{2} + 2 H_{2} O$

From the above equation it is clear that $44.8 L$ of $O_{2}$ Burns $12 g$ of carbon

Therefore the volume of oxygen required to burn $2.4 g$ of carbon completely is:

$= \frac{44.8 \times 2.4}{12}$

$= \frac{107.52}{12}$

$= 8.96 L$

Hence, the correct option is $B$

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The volume of oxygen at STP required to burn 2.4 g of carbon completely is:

The correct option is C 8.96 LCH4+2O2→CO2+2H2OFrom the above equation it is clear that 44.8L of O2 Burns 12g of carbonTherefore the volume of oxygen required to burn 2.4g of carbon completely is:=44.8×2.412=107.5212=8.96 LHence, the correct option is B

The volume of oxygen at STP required to burn $2.4$ g of carbon completely is: