Question

Calculate the amount of carbon dioxide that could be produced when
2 moles of carbon are burnt in 16g of dioxygen.

Answer 1

Step 1: Forming the balanced equation:-

The balanced chemical equation for the reaction is $\underset{\mathrm{Carbon}}{\mathrm{C}\left(\mathrm{s}\right)}+\underset{\mathrm{Oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Carbon}\mathrm{dioxide}}{{\mathrm{CO}}_2\left(\mathrm{g}\right)}$

Step 2: Dioxide is a limiting reagent:-

Here we have only 16g of oxygen(${\mathrm{O}}_2$) which corresponds to $\frac{16}{32}=0.5\mathrm{moles}$, hence dioxygen (${\mathrm{O}}_2$) here is a limiting reagent.

Step 3: Amount of carbon dioxide formed:-

As a result, it can only produce 0.5 moles of Carbon dioxide which is

$$\begin{gathered} =0.5\times \mathrm{Molecular}\mathrm{mass}\mathrm{of}\mathrm{carbon}\mathrm{dioxide}\mathrm{g} \\ =0.5\times \{12+(16\times 2\left)\right\} \\ =0.5\times 44 \\ =22\mathrm{g} \end{gathered}$$

Therefore, the amount of Carbon dioxide that could be produced when 2 moles of Carbon are burnt in 16g of dioxygen is $22\mathrm{g}$