In 1986 an electrical power plant in Taylorsville, Georgia, burned 8,376,726 ton
ID: 894284 • Letter: I
Question
In 1986 an electrical power plant in Taylorsville, Georgia, burned 8,376,726 tons of coal, a national record at that time.
A. Assuming that the coal was 84.4 % carbon by mass and that combustion was complete, calculate the number of tons of carbon dioxide produced by the plant during the year. ANSWER: 2.59 X 10^7
B. Assuming that the coal was 4.50 % sulfur by mass and that combustion was complete, calculate the number of tons of sulfur dioxide produced by the plant during the year. ANSWER: 7.53 X 10^5
C. If 56.0 % 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?
Can you please work out part B and C for me.
Explanation / Answer
b)
mass of coal = 8,376,726 tons
= 8376726*1000
= 8376726000 kg (1 ton = 1000 kg)
mass of Sulfur = 8376726000*4.5/100 = 376952670 kg
No of moles of S = 376952670*10^3 / 32
= 11779770937.5 mole
S(s) + O2(g) ---> SO2(g)
from equation:
1 mole S = 1 mole SO2
molarmass of SO2 = 64 g/mol
nO OF MOLES OF so2 = 11779770937.5 mole
mass of SO2 produced = 11779770937.5*64
= 753905.34 = 7.53*10^5 tons
c) SO2(g)+CaO(s) ----> CaSO3(s)
mass of SO2 removed = 7.53*10^5*56/100 = 421680 tons
from equation:
1 mole So2 = 1 mole caso3
No of moles of SO2 reacted = 421680*10^6 / 64 = 6588750000 mole
molarmass of CaSO3 = 120.1412 g/mol
mass ofCaSO3 Produced = 6588750000* 120.1412 = 791580331500 grams
= 791580.3 tons