20.0 g of calcium carbonate is heated to produce carbon dioxide according to the equation CaCO3(s) → CaO(s) + CO2(g)?

20.0 g of calcium carbonate is heated to produce carbon dioxide according to the equation CaCO3(s) → CaO(s) + CO2(g) If the reaction is carried out at a temperature of 800.0 degrees C and a constant pressure of 1.0 atm is maintained, what volume of carbon dioxide gas is recovered?

May 22, 2016

$C a C {O}_{3} \left(s\right) + \Delta \rightarrow C a O \left(s\right) + C {O}_{2} \left(g\right) \uparrow$

Explanation:

There are $\frac{20.0 \cdot g}{100.0 \cdot g \cdot m o {l}^{-} 1}$ $=$ $0.20 \cdot m o l \cdot C a C {O}_{3}$

Given the stoichiometry, an equivalent molar quantity of carbon dioxide gas will be evolved.

At $1$ $a t m$ pressure, and $1073 \cdot K$, this gas will have a volume of:

$V = \frac{n R T}{P}$ $=$ $\frac{0.20 \cdot m o l \times 0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1 \times 1073 \cdot K}{1 \cdot a t m}$

$=$ ??L