If the coal is burned in a power plant that uses 2000 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide? how many grams of calcium sulfite are produced daily by this power plant?

There is 86.87 tons of CaO required and there will be 186.15 tons of calcium sulfite produced.

Explanation:

Step 1: The balanced equation

S(s) + O2(g) → SO2 (l)

SO2(g) + CaO(s) → CaSO3(s)

This means 1 mol S = 1 mol SO2 = 1 mol CaO = 1 mole CaSO3

Step 2: Given data

1 ton = 907.185Kg

Molar mass of sulfur = 32.065 g/mole

Molar mass of Calcium oxide = 56.078 g/mol e

Molar mass of calcium sulfite = 120.17 g/mole

Step 3: Calculate mass of coal

2000 tons = 1802370 Kg

Step 4: Calculate mass of sulfur:

⇒ A particular coal contains 2.5% sulfur by mass.

1802370 Kg *2.5% = 45059.25 Kg = 45059250 grams

Step 5: Calculate moles of Sulfur

Moles of sulfur = mass of sulfur / Molar mass of sulfur

Moles sulfur = 45059250 grams / 32.065g/mole = 1405247.2 moles

This means there is also produced 1405247.2 moles of Calcium oxide ( CaO).

This means there is 1405247.2 * 56.078 = 78803452.5 grams = 78.803.4525 Kg = 86.8659 tons of CaO

Step 6: Calculate mass of Calcium sulfite

1405247.2 moles * 120.17 g/moles = 168868556.024 g =168868.556  kg = 186.15 tons

There is 86.87 tons of CaO required and there will be 186.15 tons of calcium sulfite produced.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.