Question

Carbondisulfide$\mathbf{\left(}\mathit{C}{\mathit{S}}_{\mathbf{2}}\mathbf{\right)}$is a liquid that is used in the production of rayon and cellophane. It is manufactured from methane and elemental sulfurvia the reaction

${\mathbf{\text{CH}}}_{\mathbf{\text{4}}}\mathbf{\text{+ 4S}}\mathbf{\to }{\mathbf{\text{CS}}}_{\mathbf{\text{2}}}{\mathbf{\text{+ 2H}}}_{\mathbf{\text{2}}}\mathbf{\text{S}}$

Calculate the mass of$\mathit{C}{\mathit{S}}_{\mathbf{2}}$that can be prepared by the complete reaction of$\mathbf{67}\mathbf{.}\mathbf{2}\mathit{g}$sulfur.

Short answer

39.5 g of carbon disulfide.

Step-by-step solution

Given reaction

Carbon disulfide is prepared by reacting methane and sulfur which gives out both carbon sulfide and hydrogen sulfide.

• The molar mass of carbon disulfide is 76.1 g/mol.
• The molar mass of sulfur is 32.1 g/mol.

Mass of carbon disulfide

According to the balanced chemical reaction, the following relations are true.

$$\begin{gathered} 4molS\to 1molC{S}_2 \\ 4\times 32.1g\to 76.1g \\ 67.2g\to ?g \end{gathered}$$

The unknown mass of the product can be calculated using the direct proportion as stated above.

The direct proportion can be solved for the mass of the product as an equation:

$$\begin{gathered} mC{S}_2=\frac{67.2}{129.4}\times 76.1 \\ =39.5g \end{gathered}$$

Therefore, we get 39.5of carbon disulfide.