Question

According to the following reaction, how many grams of carbon tetrachloride will be formed upon the complete reaction of 27.7 grams of chlorine gas with excess carbon disulfide? carbon disulfide (s) + chlorine (g) carbon tetrachloride (l) + sulfur dichloride (s) grams carbon tetrachloride

Answer 1

Answer: 15.0 g of $CCl_4$ will be formed upon the complete reaction of 27.7 grams of chlorine gas with excess carbon disulfide

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$    

$\text{Moles of} Cl_2=\frac{27.7g}{71g/mol}=0.390moles$

The balanced chemical reaction is:

$CS_2(g)+4Cl_2(g)\rightarrow CCl_4(l)+2SCl_2(s)$

$Cl_2$ is the limiting reagent as it limits the formation of product and $CS_2$ is the excess reagent.

According to stoichiometry :

4 moles of $Cl_2$ give=  1 mole of $CCl_4$

Thus 0.390 moles of  will give = $\frac{1}{4}\times 0.390=0.0975moles$ of $CCl_4$

Mass of $CCl_4=moles\times {\text {Molar mass}}=0.0975\times 154=15.0g$

Thus 15.0 g of $CCl_4$ will be formed upon the complete reaction of 27.7 grams of chlorine gas with excess carbon disulfide