# Question #a594e

Mar 23, 2017

${\text{K"_ 2"CO"_ (3(s)) -> "K"_ 2"O"_ ((s)) + "CO}}_{2 \left(g\right)}$

#### Explanation:

Potassium carbonate, ${\text{K"_2"CO}}_{3}$, will undergo thermal decomposition at temperatures that exceed ${1000}^{\circ} \text{C}$ to produce potassium oxide, $\text{K"_2"O}$, and carbon dioxiede, ${\text{CO}}_{2}$.

The balanced chemical equation that describes this decomposition reaction looks like this

${\text{K"_ 2"CO"_ (3(s)) stackrel(color(white)(acolor(red)(Delta)aaa))(->) "K"_ 2"O"_ ((s)) + "CO}}_{2 \left(g\right)}$ $\uparrow$

Notice that the chemical equation is balanced because you have $2$ atoms of potassium, $1$ atom of carbon, and $3$ atoms of oxygen on both sides of the equation.