When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction

CaCO_{3}(s) → CaO(s) + CO_{2}(g)

What is the mass of calcium carbonate needed to produce 43.0 L of carbon dioxide at STP? Express your answer with the appropriate units.

Express your answer with the appropriate units.

The ideal gas law PV = nRT relates pressure *P*, volume *V*, temperature *T*, and number of moles of a gas, *n*. The gas constant *R* equals 0.08206 L ⋅ atm/(K ⋅ mol) or 8.3145 J/(K ⋅ mol). The equation can be rearranged as follows to solve for *n*:

$\mathbf{n}\mathbf{=}\frac{\mathbf{PV}}{\mathbf{RT}}$

This equation is useful when dealing with gaseous reactions because stoichiometric calculations involve mole ratios.

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