What mass of ${\text{CO}}_{\text{2}}$ will be formed when 6g of carbon is burnt in 32g of oxygen?

The combustion reaction of carbon in presence of oxygen is

          $\text{C}\left(\text{s}\right)+{\text{O}}_{\text{2}}\left(\text{g}\right)\to {\text{CO}}_{\text{2}}\left(\text{g}\right)$

           $12\text{\hspace{0.17em}g\hspace{0.17em} \hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}}32\text{\hspace{0.17em}g\hspace{0.17em} \hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}}44\text{\hspace{0.17em}g}$

           $6\text{\hspace{0.17em}g\hspace{0.17em} \hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}}32\text{\hspace{0.17em}g\hspace{0.17em} \hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}}x\text{\hspace{0.17em}g}$

From the balanced equation it is clear that

$12\text{\hspace{0.17em}g\hspace{0.17em}of C}\to 44{\text{\hspace{0.17em}g\hspace{0.17em}of CO}}_{\text{2}}$

$6\text{\hspace{0.17em}g of C}\to x{\text{\hspace{0.17em}\hspace{0.17em}g of CO}}_{\text{2}}$

$\therefore x=\frac{6\text{\hspace{0.17em}g\hspace{0.17em}of C}}{12\text{\hspace{0.17em}g\hspace{0.17em}of C}}\times 44{\text{\hspace{0.17em}g\hspace{0.17em}of\hspace{0.17em}CO}}_2=22{\text{\hspace{0.17em}g\hspace{0.17em}of\hspace{0.17em}CO}}_2$

Here, carbon acts as the limiting reagent because least amount of product is formed in the reaction.