Question$\text{Given that the mixture contains } 0.267 \, \text{mol} \, \mathrm{N}_{2} \text{ and that the partial pressure of } \mathrm{CO}_{2} \text{ is } 0.275 \, \text{bar. Calculate the partial pressure of } \mathrm{O}_{2}.$ $P_{\mathrm{O}_{2}} = ?$ $\text{Total pressure of the mixture is } 4.67 \, \text{bar}.$

Studdy Solution
Calculate the partial pressure of $\text{O}_2$.
Substitute the known values into the rearranged equation:
$$P_{\text{O}_2} = 4.67 \, \text{bar} - P_{\text{N}_2} - 0.275 \, \text{bar}$$
Since we don't have $P_{\text{N}_2}$ directly, we assume that the remaining pressure after subtracting $P_{\text{CO}_2}$ is due to $\text{N}_2$ and $\text{O}_2$.
$$P_{\text{N}_2} + P_{\text{O}_2} = 4.67 \, \text{bar} - 0.275 \, \text{bar}$$
$$P_{\text{N}_2} + P_{\text{O}_2} = 4.395 \, \text{bar}$$
Assuming equal distribution of pressure between $\text{N}_2$ and $\text{O}_2$ (since moles of $\text{N}_2$ are given, but not for $\text{O}_2$), we have:
$$P_{\text{O}_2} = 4.395 \, \text{bar} - P_{\text{N}_2}$$
Without additional information, we cannot definitively solve for $P_{\text{O}_2}$ without knowing $P_{\text{N}_2}$.
Since the problem lacks specific information to calculate $P_{\text{N}_2}$, we cannot provide a numerical solution for $P_{\text{O}_2}$ without further data or assumptions.