A particular coal contains 2.5% sulfur by mass. When this coal is burned, the sulfur is converted into sulfur dioxide gas. The sulfur dioxide reacts with calcium oxide to form solid calcium sulfite.
If the coal is burned in a power plant that uses 1800 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide?
How many grams of calcium sulfite are produced daily by this power plant?
It's the second question I need help with. I figured out how to find the mass if CaO, which ended up being 79 tons. The reason why I put that up as well is because it may be needed to answer the second question.
So I answered the first part by doing this:
1.9979(45)=89.9055tons of SO2 a day.
0.8753(89.9055)=78.6942 which was the right answer, but then I don't know what to do from there for the second part of the question.
Can you show me step-by-step how to do it?
78.69 tons CaO x (molar mass CaSO3/molar mass CaO) = ? which is a shortcut. The long way is
78.69 tons CaO x (1 mol CaSO3/1 mol CaO) x (molar mass CaSO3/1 mol CaSO3) x (1mol CaO/molar mass CaO) = ?
By the way, you worked your part the long way too. The short way is this.
S + O2 --> SO2
SO2 + CaO ==> CaSO3
1 mol S = 1 mol SO2 = 1 mol CaO
1800 tons x 0.025 = tons S
tons S x (1 mol S/32.066g S) = mol(tons) S.
g S = mols S x molar mass CaO = tons CaO
1800 x 0.025 x (1/32) x 56.077 = 78.696 tons CaO.l
I tried to convert the tons to grams and got 7.2E7, but that ended up being wrong.
I also need a balanced equation.
So I followed that and got 168.58 and I put it as a scientific notation since it wanted only two sigfigs (1.7E2, I had to round as well), but it was wrong.
Check the problem. It asks for GRAMS, not tons.
I obtained 168.6 tons.Convert that to grams and round to two s.f.
Ah, ok. Thanks for all the help.
Still got it wrong. I converted from tons to grams, still no good.
What answer did you get for grams? I agree that 7.2E7 is not right.
168.58 tons x 2000 tons/lb x 453.6 g/lb = about 1.5E8 grams.
The equation you want is
CaO + SO2 ==> CaSO3
Yeah, I ended up getting it. It was a calculation error and I got the equations as well; I had to have two with the phases. Thanks.
To find the mass of calcium sulfite produced daily by the power plant, you will need to use stoichiometry. Here's how you can do it step-by-step:
Step 1: Determine the stoichiometric ratio between sulfur dioxide (SO2) and calcium sulfite (CaSO3) using the balanced chemical equation:
SO2 + CaO → CaSO3
From the equation, you can see that 1 mole of sulfur dioxide reacts with 1 mole of calcium sulfite.
Step 2: Convert the mass of sulfur dioxide (SO2) that you calculated (78.6942 tons) to moles.
To convert from mass to moles, you need to use the molar mass of sulfur dioxide, which is 64.07 g/mol.
78.6942 tons * (1000 kg/ton) * (1000 g/kg) / (64.07 g/mol) = X moles of SO2
Step 3: Use the stoichiometric ratio to find the moles of calcium sulfite (CaSO3).
Since the stoichiometric ratio between SO2 and CaSO3 is 1:1, the moles of SO2 will be the same as the moles of CaSO3.
X moles of SO2 = X moles of CaSO3
Step 4: Convert moles of calcium sulfite (CaSO3) to grams.
To convert from moles to grams, you need to use the molar mass of calcium sulfite, which is 136.14 g/mol.
X moles of CaSO3 * (136.14 g/mol) = Y grams of CaSO3
Therefore, Y grams of calcium sulfite are produced daily by the power plant.