A particular coal contains 2.5% sulfur by mass. When this coal is burned, the su

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

CaO(s)+SO2(g)?CaSO3(s),S(s)+O2(g)?SO2(g)

1.If the coal is burned in a power plant that uses 2300 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide? (2SIGNIFICANT FIGURES)

2.How many grams of calcium sulfite are produced daily by this power plant?(2SIGNIFICAT FIGURES)

Explanation / Answer

A)1 mol S produces 1 mol of SO2 and 1 mol of CaO is required to eliminate 1mol of SO2. As such, we need 1 mol of CaO to eliminate SO2 produced by burning 1 mol of S.

1 mol of CaO = 40+16 = 56 g

1 mol of S = 32 g

Therefore, amount of CaO required to eliminate SO2 produced by burning 32 g of S = 56 g

Hence, amount of CaO required to eliminate SO2 produced by burning 57.5 tons of S = (56 g/32 g) * 57.5 tons = 100.625 tons

The answer in two significant figure = 1.0 * 10^2 tons

(B) According to stoichiometry,

The amount of CaSO3 produced by burning 1 mol of S = 1 mol

1 mol of CaSO3 = 40+32+(16*3) = 120 g

Therefore, the amount of CaSO3 produced by burning 32 g of S = 120 g

Hence, the amount of CaSO3 produced by burning 57.5 tons of S = (120 g/32 g)* 57.5 tons = 215.625 tons = 215.625*1000*1000g = 2.15625 * 10^8 g

In two significant figures = 2.2 * 10^8g

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