# Problem: When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reactionCaCO3(s) → CaO(s) + CO2(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:n=PVRTThis equation is useful when dealing with gaseous reactions because stoichiometric calculations involve mole ratios.

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

CaCO3(s) → CaO(s) + CO2(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.

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