A coal-fired power plant bums 230 metric tons of coal that is 0 93percentage S b

Question

A coal-fired power plant bums 230 metric tons of coal that is 0 93percentage S by mass. How many metric tons of CaSO_4 could be produced in a limestone scrubber system if all of the sulfur emissions ate captured (Assume that all of the sulfur from the coal is initially converted to SO_2 which reacts with limestone and oxygen to form calcium sulfate). Response First, realize that you can work through the problem with metric tons without formally converting from metric Feedback: tons to grams and then back again. From the amount of coal and the percentage S, you can figure out the amount of S in the coal. The overall stoichiometry between S and CaSO_4 Is 1:1 There's a 5percentage tolerance in the accepted value, so normal roundoff should not affect your score.

Explanation / Answer

mass of coal = 230

mass of S = 0.93/100*230 = 2.139 tons of S

mol of S = mass/MW = 2.139 /32) = 0.006684 ton-mol of S

and we can relate S:CaSO4

mol of CaSO4 = mol of S

mol of CaSO4 = mol of S = 0.006684 ton-mol

mass of CaSO4= mol*MW = 0.006684 *136.14 = 0.9 ton of CaSO4

proposed answer is clearly incorrect, it can't be that 230 tons --> 213.9 tons are recovered, specially if S is only 0.93%

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