find mass of calcium carbonate obtaqined in reaction of 10.0g of calcium oxide with an excess of carbon dioxide
CaO + CO2 ==> CaCO3
mols CaO = grams/molar mass = ?
Use the coefficients in the balanced equation to convert mols CaO to mols CaCO3.
Now convert mols CaCO3 to grams. grams = mols CaCO3 x molar mass CaCO3
To find the mass of calcium carbonate obtained in the reaction, you need to first determine the balanced chemical equation for the reaction. The reaction between calcium oxide (CaO) and carbon dioxide (CO2) produces calcium carbonate (CaCO3):
CaO + CO2 -> CaCO3
From the balanced chemical equation, you can see that each molecule of calcium oxide reacts with one molecule of carbon dioxide to form one molecule of calcium carbonate.
Next, calculate the molar mass of calcium oxide (CaO) and calcium carbonate (CaCO3). The molar mass of an element or compound is the sum of the atomic masses of each atom in that molecule.
The atomic masses of the elements are:
Ca (calcium) = 40.08 g/mol
O (oxygen) = 16.00 g/mol
C (carbon) = 12.01 g/mol
Therefore, the molar masses are:
CaO = 40.08 g/mol + 16.00 g/mol = 56.08 g/mol
CaCO3 = 40.08 g/mol + 12.01 g/mol + (3 * 16.00 g/mol) = 100.09 g/mol
Now, use the molar mass of CaO to calculate the number of moles of CaO present in 10.0 g. To do this, divide the mass of CaO by its molar mass:
Number of moles of CaO = Mass of CaO / Molar mass of CaO
= 10.0 g / 56.08 g/mol
≈ 0.178 mol
Since the reaction occurs with an excess of CO2, the amount of CaCO3 formed will be limited by the amount of CaO available. In this case, 0.178 moles of CaO will react to form 0.178 moles of CaCO3.
Finally, calculate the mass of calcium carbonate formed by multiplying the number of moles of CaCO3 by its molar mass:
Mass of CaCO3 = Number of moles of CaCO3 * Molar mass of CaCO3
= 0.178 mol * 100.09 g/mol
≈ 17.82 g
Therefore, the mass of calcium carbonate obtained in the reaction of 10.0 g of calcium oxide with an excess of carbon dioxide is approximately 17.82 grams.