$\overline{)\frac{{\mathbf{P}}_{\mathbf{1}}}{{\mathbf{n}}_{\mathbf{1}}}{\mathbf{=}}\frac{{\mathbf{P}}_{\mathbf{2}}}{{\mathbf{n}}_{\mathbf{2}}}}$

rearrange to arrive at:

${\mathbf{n}}_{\mathbf{2}}\mathbf{=}{\mathbf{n}}_{\mathbf{1}}\mathbf{\left(}\frac{{\mathbf{P}}_{\mathbf{2}}}{{\mathbf{P}}_{\mathbf{1}}}\mathbf{\right)}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}{\mathbf{n}}_{\mathbf{2}}\mathbf{=}\mathbf{(}\mathbf{2}\mathbf{.}\mathbf{0}\mathbf{}\mathbf{mol}\mathbf{}\mathbf{CO}\mathbf{}\mathbf{+}\mathbf{}\mathbf{1}\mathbf{.}\mathbf{0}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{O}}_{\mathbf{2}}\mathbf{)}\mathbf{\left(}\frac{\mathbf{556}\mathbf{}\overline{)\mathbf{torr}}}{\mathbf{750}\mathbf{}\overline{)\mathbf{torr}}}\mathbf{\right)}$

**n _{2} = 2.224 mol**

A catalytic converter in an automobile uses a palladium or platinum catalyst to convert carbon monoxide gas to carbon dioxide according to the following reaction: 2 CO(g) + O_{2}(g) → 2 CO_{2}(g)

A chemist researching the effectiveness of a new catalyst combines a 2.0:1.0 mole ratio mixture of carbon monoxide and oxygen gas (respectively) over the catalyst in a 2.45-L flask at a total pressure of 750 torr and a temperature of 552˚C. When the reaction is complete, the pressure in the flask has dropped to 556 torr. What percentage of the carbon monoxide was converted to carbon dioxide?

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