Question

A $6.0g$ sample of carbon is burned to produce carbon dioxide. The yield from the reaction is only $60$%.
How much carbon dioxide was actually produced?

Answer 1

$6.0g$ of carbon is burned to produce $C{O}_2$.

$C+O_2⟶C{O}_{2}1mole1mole12g44g$

$12g$ of $C$ produces $44g$ of $C{O}_2$.

$\therefore 6.0g$ of $C$ produces $\frac{44\times 6.0}{12}=22g$ of $C{O}_2$.

Percentage yield$=60\%$

Hence actually produced $C{O}_2$ $=22\times 0.6=13.2g$