Question

Carbon reacts with chlorine to form $CC{l}_{4.}$ 36gm of carbon was mixed with 142 gm of $C{l}_{2.}$ Then the mass of $CC{l}_4$ produced and the remaining mass of reactant is:

• A. $w_{CC{l}_4}=154gm,w=24gm$
• B. $w_{CC{l}_4}=156gm,w=24gm$
• C. $w_{CC{l}_4}=56gm,w=29gm$
• D. $w_{CC{l}_4}=269gm,w=549gm$

Answer 1

The correct option is A $w_{CC{l}_4}=154gm,w=24gm$

The balanced chemical reaction is $C+2C{l}_2\to CC{l}_4$
36 g of carbon will react with $\frac{36}{12}\times 2\times 71=426g$ of chlorine.
However only 142 g of chlorine are present.
Thus chlorine is the limiting reagent.
142 g of chlorine will produce $\frac{142\times 154}{71\times 2}=154g$ of carbon tetrachloride.
142 g (2 moes) of chlorine will react with 12 g (1 mole) of carbon.
The amount of carbon remaining unreacted after the reaction is $36-12=24g$