What volume of $\mathrm{CO}_{2(\mathrm{~g})}$ at STP is obtained by complete combustion of $6 \mathrm{~g}$…
What volume of $\mathrm{CO}_{2(\mathrm{~g})}$ at STP is obtained by complete combustion of $6 \mathrm{~g}$ carbon?
- $22.4 \mathrm{dm}^3$
- $11.2 \mathrm{dm}^3$
- $5.6 \mathrm{dm}^3$
- $2.24 \mathrm{dm}^3$
Solution
$\begin{array}{ll} & \mathrm{C}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \longrightarrow \mathrm{CO}_{2(\mathrm{~g})} \\ & 1 \mathrm{~mol} \mathrm{C} \equiv 1 \mathrm{~mol} \mathrm{CO}_{2(\mathrm{~g})} \\ & 6 \mathrm{~g} \mathrm{C}=0.5 \mathrm{~mol} \mathrm{C} \\ \therefore \quad & 0.5 \mathrm{~mol} \mathrm{C} \equiv 0.5 \mathrm{~mol} \mathrm{CO}_{2(\mathrm{~g})} \\ & \text { At STP, } 1 \mathrm{~mol} \mathrm{CO}_{2(\mathrm{~g})}=22.4 \mathrm{dm}^3 \\ \therefore \quad & 0.5 \mathrm{~mol} \mathrm{CO} 2(\mathrm{~g})=11.2 \mathrm{dm}^3\end{array}$
Asked in: MHT CET 2023 (12 May Shift 1)
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