Consider using two balanced chemical equations to describe this reaction:

- 2S + Cl
_{2}→ S_{2}Cl_{2} - S + Cl
_{2}→ SCl_{2}

Because this mixture of **S and Cl _{2} reacts completely**,

Let: *m _{1} = mass of S , m_{2} = mass of Cl*

$\mathbf{m}\mathbf{=}\frac{{\mathbf{m}}_{\mathbf{1}}}{\mathbf{32}\mathbf{.}\mathbf{07}}\mathbf{-}\frac{{\mathbf{m}}_{\mathbf{2}}}{\mathbf{35}\mathbf{.}\mathbf{45}\mathbf{\times}\mathbf{2}}\mathbf{(}\mathbf{35}\mathbf{.}\mathbf{45}\mathbf{\times}\mathbf{2}\mathbf{+}\mathbf{32}\mathbf{.}\mathbf{07}\mathbf{\times}\mathbf{2}\mathbf{)}$

A mixture of 56.0 g of S and 1.06×10^{2} g of Cl_{2} reacts completely to form S_{2}Cl_{2} and SCl_{2}.

Find the mass of S_{2}Cl_{2} formed.

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