Question #a594e

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Question #a594e

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Answer 1 · 2017-03-23T01:20:51

$K_{2} {CO}_{3 (s)} \to K_{2} O_{(s)} + {CO}_{2 (g)}$ $"K"_ 2"CO"_ (3(s)) -> "K"_ 2"O"_ ((s)) + "CO"_ (2(g))$

Explanation:

Potassium carbonate, $K_{2} {CO}_{3}$ $"K"_2"CO"_3$ , will undergo thermal decomposition at temperatures that exceed $1000^{\circ} C$ $1000^@"C"$ to produce potassium oxide, $K_{2} O$ $"K"_2"O"$ , and carbon dioxiede, ${CO}_{2}$ $"CO"_2$ .

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

$"K"_ 2"CO"_ (3(s)) stackrel(color(white)(acolor(red)(Delta)aaa))(->) "K"_ 2"O"_ ((s)) + "CO"_ (2(g))$ $uarr$

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.

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