100 g of propane is completely reacted with 1000 g of oxygen.
Question:

$100 \mathrm{~g}$ of propane is completely reacted with $1000 \mathrm{~g}$ of oxygen. The mole fraction of carbon dioxide in the resulting mixture is $x \times 10^{-2}$. The value of $x$ is__________ (Nearest integer)

[Atomic weight : $\mathrm{H}=1.008 ; \mathrm{C}=12.00 ; \mathrm{O}=16.00]$

Solution:

$\mathrm{C}_{3} \mathrm{H}_{8(\mathrm{~g})}+5 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 3 \mathrm{CO}_{2(\mathrm{~g})}+4 \mathrm{H}_{2} \mathrm{O}_{(\ell)}$

$\mathrm{t}=0 \quad 2.27$ mole $31.25 \mathrm{~mol}$

$\mathrm{t}=\infty \quad 0 \quad 19.9 \mathrm{~mol} \quad 6.81 \mathrm{~mol} \quad 9.08 \mathrm{~mol}$

mole fraction of $\mathrm{CO}_{2}$ in the final reaction mixture (heterogenous)

$\mathrm{X}_{\mathrm{CO}_{2}}=\frac{6.81}{19.9+6.81+9.08}$

$=0.1902=19.02 \times 10^{-2}$

$\Rightarrow 19$

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