Carbon disulphide $\left(C{S}_2\right)$ can be made from by product $S{O}_2$. The overall reaction is as follows:
$5C+2S{O}_2\to C{S}_2+4CO$
How much $C{S}_2$ can be produced from $450$ kg of waste $S{O}_2$ with excess of coke if the $S{O}_2$ conversion is $82\%$?

The correct option is A $219$
The molar mass of $S{O}_2$ is $32+2\left(16\right)=64$ g/mol
The molar mass of $C{S}_2$ is $12+2\left(32\right)=76$ g/mol
$2$ moles of $S{O}_2$ form $1$ mole of $C{S}_2$.
$2\times 64=128$ g of $S{O}_2$ form $76$ g of $C{S}_2$.
$450$ kg of $S{O}_2$ will form $\frac{76}{128}\times 450=267$ kg of $C{S}_2$.
However, the conversion is only $82\%$.
Hence, $\frac{82}{100}\times 267=219$ kg of $C{S}_2$ will be formed.