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.

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=PVRT

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

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.