If 10.11 g of limestone decomposes by heat to give 8.51 g of solid calcium oxide and carbon dioxide gas, what is the mass of carbon dioxide produced?
I ASSUME the 8.51g is the mass of the CaO and NOT the combined mass of CaO + CO2. The way the problem is stated makes one think the sum of the two is 8.51g.
CaCO3 ==> CaO + CO2
Mass CO2 = loss in weight = 10.11-8.51 = 1.6g.
mols CO2 = grams/molar mass = ?
From the equation you can see that mols CO2 = mols CaCO3.
Convert mols CO2 to mols CaCO3 then to g CaCO3
Then (g CaCO3/10.11)*100 = ?% CaCO3
To find the mass of carbon dioxide produced, we need to calculate the difference in mass between the reactant (limestone) and the product (solid calcium oxide):
Mass of calcium oxide = 8.51 g
Mass of limestone = 10.11 g
To find the mass of carbon dioxide produced, we need to subtract the mass of calcium oxide from the mass of limestone:
Mass of carbon dioxide = Mass of limestone - Mass of calcium oxide
Mass of carbon dioxide = 10.11 g - 8.51 g
Mass of carbon dioxide = 1.60 g
Therefore, the mass of carbon dioxide produced is 1.60 g.
To find the mass of carbon dioxide produced, we need to determine the mass difference between the initial mass of limestone and the final mass of solid calcium oxide.
Step 1: Calculate the mass of carbon dioxide produced from the given data.
- The mass of limestone is 10.11 g.
- The mass of solid calcium oxide is 8.51 g.
Step 2: Determine the mass difference between the limestone and calcium oxide.
Mass difference = Mass of limestone - Mass of calcium oxide
Mass difference = 10.11 g - 8.51 g
Mass difference = 1.60 g
Therefore, the mass of carbon dioxide produced is 1.60 g.