Question

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 solid calcium oxide to form solid calcium sulfite.

Answer 1

1) S(s)+O2(g) ->SO2(g),SO2(g)+CaO(g) ->CaSO3(s)

Answer 2

2)1800 tons of coal contains 2.5% sulfur. Thus, S(s) content is 2.5%*1800 = 45.0 tons.

tons corresponds to weight. therefore, we need to find how many moles of S(s) is used daily.

molecular weight of S = 32.06g/mol.
moles present = 45.0/32.06 = 1.404 moles *tons/grams

1 mole of sulfur is needed to make 1 mole of SO2(g). Therefore, the moles of SO2(g) = moles of S(g) = 1.404 moles *tons/grams

TO eliminate 1mole of SO2(g), we require 1mole of CaO(s) ---chemical reaction 2

1mole of CaO = 1 mole of SO2 =1.404 moles *tons/grams

Now, we find the weight of CaO needed

molecular weight of CaO = 56.08g/mol