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.

Part A

Write the balanced chemical equations for the reactions.

Express your answers as chemical equations separated by a comma. Identify all of the phases in your answer.

Part B

If the coal is burned in a power plant that uses 2100 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide?

Express your answer using two significant figures

Part C

How many grams of calcium sulfite are produced daily by this power plant?

Express your answer using two significant figures.

Part C

How many grams of calcium sulfite are produced daily by this power plant?

Express your answer using two significant figures.

Explanation / Answer

A)
CaO (s) + SO2 (g)   ---> CaSO3 (s)

B)
mass of coal = 2100 tons = 2,100,000 kg

mass of S = 2.5 % of 2,100,000 kg
= 5.25*10^4 kg
= 5.25*10^7 g

mol of S = mass/molar mass
= (5.25*10^7)/(32)
=1.64*10^3 mol

so, moles of SO2 formed = 1.64*10^3 mol

hence, moles of CaO required = 1.64*10^3 mol

molar mass of CaO = 56.1 g/mol

mass of CaO = molar mass * number of mol
= 56.1 g/mol * 1.64*10^3 mol
= 9.2*10^4 g

Answer: 9.2*10^4 g

C)
mol of CaSO3 formed = 1.64*10^3 mol
molar mass of CaSO3 = 120 g/mol

mass of CaSO3 formed = number of mol * molar mass
= 1.64*10^3 mol * 120 g/mol
= 2.0*10^5 g

Answer: 2.0*10^5 g

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