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A particular coal contains 2.5% sulfur by mass. When this coal is burned at a power plant, the sulfur is converted into sulfur dioxide gas, which is a pollutant. To reduce sulfur dioxide emissions, calcium oxide (lime) is used. The sulfur dioxide reacts with calcium oxide to form solid calcium sulfite. (a) Write the balanced chemical equation for the reaction. (b) If the coal is burned in a power plant that uses 2000 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide? (c) How many grams of calcium sulfite are produced daily by this power plant?

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Jamar Ferry
Jamar FerryLv2
29 May 2020

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Related questions

When coal is burned, the sulfur it contains is converted into sulfur dioxide. This 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 1893 kg of SO2 removed by this technique

Acertain sample of coal contains 1.2% sulfur by mass. When the coalis burned, the sulfur is converted to sulfur dioxide(SO2). To preventair pollution, SO2is treated with calcium oxide (CaO) to form calcium sulfite(CaSO3) as shownin the reaction below


SO2(g) + CaO(s) -->CaSO3(s)


Calculate the daily mass (in kilograms) of CaO needed by a powerplant that uses 6.60

Coal is a fossil fuel made primarily of carbon, but it also contains sulfur among other elements.

When carbon, C, burns in air, it reacts with oxygen, O2, to produce carbon dioxide,CO2:

C(s)+O2(g)→CO2(g)

When sulfur, S, burns in air, it reacts with oxygen, O2, to produce sulfur dioxide, SO2:

S(s)+O2(g)→SO2(g)

In 1986 an electrical power plant in Taylorsville, Georgia, burned 8,376,726 tons of coal, a national record at that time.

Part A

Assuming that the coal was 87.4 % carbon by mass and that combustion was complete, calculate the number of tons of carbon dioxide produced by the plant during the year.

Part B

Assuming that the coal was 3.10 % sulfur by mass and that combustion was complete, calculate the number of tons of sulfur dioxide produced by the plant during the year.

Part C

If 63.0 % of the SO2 could be removed by reaction with powdered calcium oxide, CaO, via the reaction

SO2(g)+CaO(s)→CaSO3(s)

how many tons of calcium sulfite, CaSO3, would be produced?

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