Question

$100$ ml of nitrogen at $0.30$ atm, pressure and $50$ ml of carbon dioxide at $0.60$ atm. pressure are introduced into a vessel of volume $150$ ml without any change in temperature. What will be ratio of the partial pressure of nitrogen to carbon dioxide in the vessel?

• A. $1:2$
• B. $2:1$
• C. $1:1$
• D. $1:3$

Answer 1

The correct option is C $1:1$

The ratio of the partial pressure of nitrogen to carbon dioxide in the vessel will be equal to the ratio of the number of nitrogen to carbon dioxide. It will be equal to the ratio of the product of the pressure and volume of nitrogen to carbon dioxide .
$P_{\text{nitrogen}}:P_{\text{carbon dioxide}}=P_{\text{nitrogen}}^o\times V_{\text{nitrogen}}^o:P_{\text{carbon dioxide}}^o\times V_{\text{carbon dioxide}}^o=\text{0.30 atm}\times \text{100 mL}:\text{0.60 atm}\times \text{50 mL}=1:1$
Note: $P_{\text{nitrogen}}$ and $P_{\text{carbon dioxide}}$ are final pressures.
$P_{\text{nitrogen}}^o$ and $P_{\text{carbon dioxide}}^o$ are initial pressures.
$V_{\text{nitrogen}}^o$ and $V_{\text{carbon dioxide}}^o$ are initial volumes.