What volume of CO2 at $27^{\circ} C$ and 700 mm pressure will be formed when 100mL of carbon monoxide at $127^{\circ} C$ and 725 mm is completely oxidized with oxygen gas?

Question

What volume of $CO _{2}$ at $27^{\circ} C$ and $700 mm$ pressure will be formed when $100 mL$ of carbon monoxide at $127^{\circ} C$ and $725 mm$ is completely oxidised with oxygen gas?

Answer 1

SOLUTION : $\quad 2 CO ( g )+ O _{2}( g )=2 CO _{2}( g )$

$\begin{array}{ll}2 \text { vol } & 2 \text { vol. } \\ 100 mL & 100 mL \end{array}$

Since the same vol. of $CO _{2}$ is formed from the same volume of $CO$, hence the volume of $CO _{2}$ formed at $127^{\circ} C$ and $725 mm$ pressure (according to Gay-Lussac's law) from 100.

Now,

By ideal gas cquation, $\frac{P_{1} V_{1}}{T_{1}}=\frac{P_{2} V_{2}}{T_{2}}$

$\therefore \quad V_{2}=\frac{P_{1} V_{1}}{T_{1}} \times \frac{T_{2}}{P_{2}}=\frac{725 \times 100}{400} \times \frac{300}{700} mL =77 \cdot 7 mL \text {. }$