CaCO3 --- CaO+CO2 the mass of CaCO3 that must be decomposed to give 22g of CO2
Ca = 112.4 g/mol
C = 12 g/mol
O = 16 g/mol
so
CaCO3 = 112.4+ 12 + 48 = 172.4 g/mol
CO2 = 12 + 32 = 44 g/mol
same mols of each
22 g CO2 * 1 mol / 44g = 1/2 mol
1/2 mol of CaCO3 = (1/2)(172.4 ) = 86.2 grams of CaCO3
@ Anonymous. oops. Ca is 40.1. CaCO3 is a nice round number like 100 g/mol. So the method is OK but not the numbers. Tried to think how you got 112 but couldn't.
To determine the mass of CaCO3 that must be decomposed to give 22 g of CO2, we need to use the given balanced chemical equation:
CaCO3 → CaO + CO2
From the equation, we can see that the molar ratio between CaCO3 and CO2 is 1:1. This means that for every one mole of CaCO3, one mole of CO2 is produced.
To find the mass of CaCO3, we need to calculate the molar mass of CO2. The molar mass of CO2 is the sum of the molar masses of carbon (C) and two oxygen (O) atoms:
C: 12.01 g/mol
O: 16.00 g/mol
(2 x O) = 2 x 16.00 g/mol = 32.00 g/mol
Molar mass of CO2 = 12.01 g/mol + 32.00 g/mol = 44.01 g/mol
Now, we can set up a proportion to find the mass of CaCO3:
Mass of CaCO3 / Molar mass of CaCO3 = Mass of CO2 / Molar mass of CO2
Let's plug in the values:
Mass of CaCO3 / 100.09 g/mol = 22 g / 44.01 g/mol
Cross-multiplying, we get:
Mass of CaCO3 = (22 g / 44.01 g/mol) x 100.09 g/mol
Mass of CaCO3 = 49.960 g
Therefore, approximately 49.960 grams of CaCO3 must be decomposed to give 22 g of CO2.
To determine the mass of CaCO3 that must be decomposed to produce 22g of CO2, we need to use the balanced chemical equation and stoichiometry.
The balanced chemical equation for the decomposition of CaCO3 is:
CaCO3 → CaO + CO2
According to the equation, one mole of CaCO3 decomposes to produce one mole of CO2. The molar mass of CaCO3 is calculated by adding up the atomic masses of calcium (Ca), carbon (C), and three oxygen (O) atoms:
CaCO3 = 40.08 g/mol (Ca) + 12.01 g/mol (C) + (16.00 g/mol x 3) (O) = 100.09 g/mol
Now, we can calculate the number of moles of CO2 produced by using its molar mass. The molar mass of CO2 is:
CO2 = 12.01 g/mol (C) + (16.00 g/mol x 2) (O) = 44.01 g/mol
Using the equation:
Mass of CO2 (g) = Number of moles of CO2 x Molar mass of CO2 (g/mol)
Rearranging the equation to solve for the number of moles of CO2:
Number of moles of CO2 = Mass of CO2 (g) / Molar mass of CO2 (g/mol)
Number of moles of CO2 = 22 g / 44.01 g/mol = 0.5 mol
Since the balanced chemical equation shows that the ratio between CaCO3 and CO2 is 1:1, the number of moles of CaCO3 decomposed is also 0.5 mol.
Now, we can calculate the mass of CaCO3 using its molar mass:
Mass of CaCO3 = Number of moles of CaCO3 x Molar mass of CaCO3
Mass of CaCO3 = 0.5 mol x 100.09 g/mol = 50.05 g
Therefore, the mass of CaCO3 that must be decomposed to produce 22g of CO2 is approximately 50.05 grams.