When coal is burned, the sulfur it contains is converted into sulfur dioxide. This is SO2 is a serious pollutant, so it needs to be removed before it escapes from the stack of a coal fired plant. One way to remove the SO2 is to add limestone, which contains calcium carbonate, CaCO3, to the coal before it is burned. The heat of the burning coal converts the CaCo3 to calcium oxide, CaO. The calcium oxide reacts with the sulfur dioxide in the following reaction:
2CaO+2SO2+O2=2CaSO4
The solid calcium sulfate does not escape from the stack as the gaseous sulfur dioxide would. What mass of calcium sulfate forms for each 1.00 Mg (Megagram) of SO2 removed by this technique?
Joe/Jimmy/Marissa -- please use the same name for all of your posts.
Ms. Sue is right. You get faster and better help if you don't change screen names.
2CaO + 2SO2 + O2=> 2CaSO4
mols SO2 - 1E6/molar mass SO2 = ?
Using the coefficients in the balanced equation, convert mols SO2 to mols CaSO4.
Now convert mols CaSO4 to grams. g CaSO4 = mols CaSO4 x molar mass CaSO4.
How do you know she/he changed screen names. ALSO: To "Marissa". Ms. Sue is correct. If you did change screen names, that's a problem because you seem to be both a boy and a girl which may confuse people and distract them from answering. (Joe & Jimmy are boy names and Marissa is a girl name)
It seems several students think by using both boys and girls names we will think they are different people. Not so. How do we know the same person is using different screen names. Easy. The IP address, which shows when the question/response is posted, tells us the computer being used. We can also tell where it is in most cases.
Sorry were working in a group and not everyone has the same questions and so we know who's question is which
sorry for the confusion !
To determine the mass of calcium sulfate formed, we need to use stoichiometry and the molar mass of calcium sulfate.
1. Convert the mass of SO2 from Megagrams (Mg) to grams:
1.00 Mg = 1.00 x 10^6 grams (1 Mg = 10^6 grams)
2. Convert the mass of SO2 to moles using the molar mass of SO2:
Molar mass of SO2 = 32.06 g/mol (sulfur: 32.06 g/mol, oxygen: 16.00 g/mol x 2)
Moles of SO2 = (mass of SO2 in grams) / (molar mass of SO2)
3. Use the balanced chemical equation to determine the mole ratio between CaO and SO2:
According to the reaction: 2CaO + 2SO2 + O2 → 2CaSO4
The mole ratio is 2:2, which means 2 moles of CaO react with 2 moles of SO2 to form 2 moles of CaSO4.
4. Calculate the moles of CaSO4 formed by multiplying the moles of SO2 by the mole ratio:
Moles of CaSO4 = Moles of SO2
5. Convert the moles of CaSO4 to grams using the molar mass of CaSO4:
Molar mass of CaSO4 = 136.14 g/mol (calcium: 40.08 g/mol, sulfur: 32.06 g/mol, oxygen: 16.00 g/mol x 4)
Mass of CaSO4 = Moles of CaSO4 x Molar mass of CaSO4
Substituting the values into the equations:
1. Mass of SO2 = 1.00 x 10^6 grams
2. Moles of SO2 = (1.00 x 10^6 grams) / (32.06 g/mol) = 3.12 x 10^4 moles
3. Moles of CaSO4 = 3.12 x 10^4 moles
4. Mass of CaSO4 = (3.12 x 10^4 moles) x (136.14 g/mol) = 4.25 x 10^6 grams
Therefore, for every 1.00 Mg of SO2 removed by this technique, approximately 4.25 x 10^6 grams (or 4.25 x 10^3 kilograms) of calcium sulfate would be formed.