Question

Complete and balance the following chemical equation:

$\mathrm{\_}+6.5{\mathrm{O}}_2\to 4{\mathrm{CO}}_2+5{\mathrm{H}}_2\mathrm{O}+\mathrm{Heat}$

Answer 1

A combustion reaction occurs when fuel is oxidized by reacting with an oxidizing agent and releasing energy is called combustion reaction.

The combustion reaction of Butane $\left({\mathrm{C}}_4{\mathrm{H}}_{10}\right)$ in the presence of $6.5$ moles of Oxygen $\left({\mathrm{O}}_2\right)$ forms four moles of Carbon dioxide $\left({\mathrm{CO}}_2\right)$ and five moles of Water $\left({\mathrm{H}}_2\mathrm{O}\right)$ with the generation of heat.

The complete and balanced chemical equation of the combustion reaction of Butane is written as:

$$\begin{gathered} {\mathrm{CH}}_3-{\mathrm{CH}}_2-{\mathrm{CH}}_2-{\mathrm{CH}}_3+6.5{\mathrm{O}}_2\to 4{\mathrm{CO}}_2+5{\mathrm{H}}_2\mathrm{O}+\mathrm{Heat} \\ \left(\mathrm{Butane}\right)\left(\mathrm{Oxygen}\right)(\mathrm{Carbon}(\mathrm{Water}) \\ \mathrm{dioxide}) \end{gathered}$$