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.
1)Write the balanced chemical equation for the reaction.
2)If the coal is burned in a power plant that uses 1800 short tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide?
3)How many grams of calcium sulfite are produced daily by this power plant?
I would appreciate the help, I'm lost and don't understand this. If you could explain the answer, I'd be grateful.
1)Write the balanced chemical equation for the reaction.
2)If the coal is burned in a power plant that uses 1800 short tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide?
3)How many grams of calcium sulfite are produced daily by this power plant?
I would appreciate the help, I'm lost and don't understand this. If you could explain the answer, I'd be grateful.
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C + O2 = CO2
S + O2 = SO2
CaCO3 + SO2 → CaSO3 +
CO2
or maybe
Ca(OH)2 + SO2 → CaSO3
+ H2O
2.5% of 2000 tons = 50
tons of sulfur.
Each mole of S produces
one mole of CaSO3.
So the weight of CaSO3
produced is 50 tons
times the ratio of the
molecular weights of
CaSO3 and S:
50 (120.1422 /
32.0655 ) = 187 tons of
CaSO3
S + O2 = SO2
CaCO3 + SO2 → CaSO3 +
CO2
or maybe
Ca(OH)2 + SO2 → CaSO3
+ H2O
2.5% of 2000 tons = 50
tons of sulfur.
Each mole of S produces
one mole of CaSO3.
So the weight of CaSO3
produced is 50 tons
times the ratio of the
molecular weights of
CaSO3 and S:
50 (120.1422 /
32.0655 ) = 187 tons of
CaSO3