MCQ
If isobutane and $n-$ butane are present in a gas, then how much oxygen should be required for complete combusition of $10\,kg$ of this gas ........... $\mathrm{kg}$
- ✓$35.862$
- B$9$
- C$27$
- D$1.8$
✓
Answer
Correct option: A.
$35.862$
a
Isobutane and $n$ -Butane have same chemical formula $\left(C_{4} H_{10}\right)$ and give same combustion reaction.
Isobutane and $n$ -Butane have same chemical formula $\left(C_{4} H_{10}\right)$ and give same combustion reaction.
$2 C_{4} H_{10}+13 O_{2} \rightarrow 8 C O_{2}+10 H_{2} O$
This means $2$ moles of this mixture requires $13$ moles of oxygen.
Molecular mass of butane $=58 g / m o l$
Molecular mass of oxygen $=32 g / m o l$
Moles of butane in $10 k g=\frac{10 \times 1000}{58}=\frac{10000\times 13}{58\times 2}$ moles of $O_{2}=\frac{130000\times 32}{116} g$
$O_{2}=\frac{130 \times 32}{116}\, k g\, O_{2}$
Therefore, $35.862 \,\mathrm{kg}$ oxygen is used.
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