# If 500,000g of limestone is heated up, what is the mass of CaO? CaCO3 = CaO + CO2

May 27, 2017

Well we have the stoichiometric equation........and we get over $280$ $\text{kg}$ of calcium oxide..........

#### Explanation:

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

And, clearly, there is 1:1 molar relationship between the limestone and calcium oxide product........

$\text{Moles of calcium carbonate} = \frac{500 \times {10}^{3} \cdot g}{100.09 \cdot g \cdot m o {l}^{-} 1} = 5.00 \times {10}^{2} \cdot m o l$

$\text{Mass of calcium oxide} = 5.00 \times {10}^{3} \cdot m o l \times 56.08 \cdot g \cdot m o {l}^{-} 1$

$= 280.1 \times {10}^{3} \cdot g \equiv 280$ $\text{kg}$

For what would we typically use this quantity of $\text{quicklime}$?