# Problem: A mixture of 56.0 g of S and 1.06×102 g of Cl2 reacts completely to form S2Cl2 and SCl2.Find the mass of S2Cl2 formed.

###### FREE Expert Solution

Consider using two balanced chemical equations to describe this reaction:

• 2S + Cl2 → S2Cl2
• S + Cl2 → SCl2

Because this mixture of S and Cl2 reacts completely, no molecular S and Cl2 remain when the reaction is complete. Treat the two balanced equations as a system of equations where one equation can be substituted into the other to solve for one of the two unknown quantities.

Let: m1 = mass of S , m2 = mass of Cl2

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

###### Problem Details

A mixture of 56.0 g of S and 1.06×102 g of Cl2 reacts completely to form S2Cl2 and SCl2.

Find the mass of S2Cl2 formed.