Chapter 6, Problem 6.113QP

Interpretation Introduction

Interpretation: The final pressure in the flask when carbon monoxide at $\text{680}\text{mm}\text{Hg}$ reacts with ${\text{O}}_{\text{2}}$ at $\text{340}\text{mm}\text{Hg}$ to produce ${\text{CO}}_{\text{2}}$ is to be calculated.

Concept introduction: The balanced chemical reaction between carbon monoxide and ${\text{O}}_{\text{2}}$ is written below,

$\text{2CO}\left(\text{g}\right)+{\text{O}}_{\text{2}}\left(\text{g}\right)\to {\text{2CO}}_{\text{2}}\left(\text{g}\right)$

The above reaction shows that number of moles of ${\text{O}}_{\text{2}}$ is half than the number of moles of $\text{CO}$. None of the reagents is a limiting reactant in the above reaction as both $\text{CO}$ and ${\text{O}}_{\text{2}}$ completely react to make moles of ${\text{CO}}_{\text{2}}$ for every single mole of $\text{CO}$. As both the temperature and volume are constant for both the gases, this means that the pressure is directly depends upon the number of moles.

To calculate: The final pressure in the flask when carbon monoxide at $\text{680}\text{mm}\text{Hg}$ reacts with ${\text{O}}_{\text{2}}$ at $\text{340}\text{mm}\text{Hg}$ to produce ${\text{CO}}_{\text{2}}$.