Calculate the volume of oxygen required to burn completely \(20 \mathrm{~cm}^3\) of Carbon (II) oxide.
A. \(10 \mathrm{~cm}^3\) B. \(20 \mathrm{~cm}^3\) C. \(30 \mathrm{~cm}^3\) D. \(40 \mathrm{~cm}^3\)
Correct Answer: A
Explanation
\(2 \mathrm{CO}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}\) \(20 \mathrm{~cm}^3: 10 \mathrm{~cm}^3: 20 \mathrm{~cm}^3\) Thus, \(20 \mathrm{~cm}^3\) of \(\mathrm{CO}\) will burn in \(10 \mathrm{~cm}^3\) of \(\mathrm{O}_2\) to produce \(20 \mathrm{~cm}^3\) of \(\mathrm{CO}_2\)
