Question

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 81.4 % carbon by mass and that combustion was complete, calculate the number of tons of carbon dioxide produced by the plant during the year. In 1986 an electrical power plant in Taylorsville, Georgia, burned 8,376,726 tons of coal, a national record at that time.

Part B Assuming that the coal was 2.10 % 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 73.0 % 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?

Answer 1

GIven

Mass of Coal = 8376726 tons

Given coal contains 81.4 % of Carbon

so Mass of carbon = 8376726 tons * 0.814 = 6818654.964 tons = 6818654964 kg

Molar mass of C = 12 kg/kmol

No. of moles of C = 6818654964 kg / 12 kg/kmol = 568221247 kmol

C + O2 ---> CO2

1 mole of C on combustion will give one mole of CO2

so No. of moles of CO2 produced = 568221247 kmol

Molar mass of CO2 = 44 kg/kmol

mass of CO2 produced = 568221247 kmol * 44 kg/kmol = 25001734870 kg = 25001734.87 tons Answer (A)

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Given mass of sulfur is 2.1% in coal

Molar mass of S = 32 g/mol

Molar mass of SO2 = 64 g/mol

S + O2 ---> SO2

One mole of S gives one mole of SO2

Mass of SO2 produced = (mass of coal * 0.021) * 64 g/mol / 32 g/mol = 351822.492 tons Answer (B)

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Given reaction for SO2

SO2(g)+CaO(s)→CaSO3(s)

1 mole 1mole

64 g/mol 100 g/mol

73 % of SO2 is converted to CaSO3

Mass of CaSO3 = (Mass of SO2 produced * 0.73) * 100 g/mol / 64 g/mol = 401297.53 tons Answer (C