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The combustion of pure sulfur can proceed by either of the following reactions:

$$S(s)+{ O }_{ 2 }(g)\xrightarrow [ ]{ } { SO }_{ 2 }(g)$$

$$2S(s)+{ 3O }_{ 2 }(g)\xrightarrow [ ]{ } { 2SO }_{ 3 }(g)$$

If 3.0 moles of $S(s)$ react completely with 10.0 moles of ${O }_{ 2 }(g)$ and 1.0 mole of ${ SO }_{ 3 }(g)$ is produced, what is the partial pressure of the ${ SO }_{ 3 }(g)$ given that the total pressure inside the reaction chamber is 8 atm following the combustion reaction?

A

${1.25\text{ atm}}$

B

${0.80\text{ atm}}$

C

${0.84\text{ atm}}$

D

${0.96\text{ atm}}$

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