$NCERT$ Class $XI^{th}$ Page $220 .$ Question $7.23$ Let total mass of gaseous mixture be $100\, \mathrm{gm}$. mass of $\mathrm{CO}_{(\mathrm{g})}=84 \, \mathrm{gm}$ and mass of
$\mathrm{CO}_{2(\mathrm{s})}=(100-84) \mathrm{gm}=16\, \mathrm{gm}$
Moles of $\mathrm{CO}_{(\mathrm{g})}=\frac{84}{28}=3$
mole of $\mathrm{CO}_{2}=\frac{16}{44}=0.36$
Partial pressure of $\mathrm{CO}=\frac{3}{3.36} \times 2=1.785\, \mathrm{atm}$
Partial pressure of $\mathrm{CO}_{2}=\frac{0.36}{3.36} \times 2=0.214\, \mathrm{atm}$
$\mathrm{K}_{\mathrm{p}}=\frac{\left(\mathrm{P}_{\mathrm{CO}}\right)^{2}}{\left(\mathrm{P}_{\mathrm{CO}_{2}}\right)}=\frac{(1.785)^{2}}{(0.214)}=14.89\, \mathrm{atm}$
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$C{H_{4(g)}} + 2{O_{2(g)}} \to C{O_{2(g)}} + 2{H_2}{O_{(g)}}$