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Question

Trace amounts of sulfur (S) in coal are burned in the presence of diatomic oxygen $\left(O_{2}\right)$ to form sulfur dioxide $\left(S O_{2}\right).$ Determine the minimum mass of oxygen required in the reactants and the mass of sulfur dioxide in the products when 1 kg of sulfur is burned.

Solution

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The solutions are obtained from the molar mass ratios of the components of the reaction:

\begin{align*} \dfrac{m_{\text{O}_{2}}}{m_{\text{S}}}&=\dfrac{M_{\text{O}_{2}}}{M_{\text{S}}}\\ &=\dfrac{32}{32.063}\\ &=\boxed{\dfrac{0.998\:\text{kg}\:\text{O}_{2}}{1\:\text{kg}\:\text{S}}} \end{align*}

\begin{align*} \dfrac{m_{\text{SO}_{2}}}{m_{\text{S}}}&=\dfrac{M_{\text{SO}_{2}}}{M_{\text{S}}}\\ &=\dfrac{64.063}{32.063}\\ &=\boxed{\dfrac{1.998\:\text{kg}\:\text{O}_{2}}{1\:\text{kg}\:\text{S}}} \end{align*}

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