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Sulfur dioxide is a toxic gas that is admitted into the atmosphere from volcanic irruption's as...

Sulfur dioxide is a toxic gas that is admitted into the atmosphere from volcanic irruption's as well as from human activities such as coal burning. Sulfur dioxide canreact with water in the atmosphere to form sulfuric acid, a key component in acid rain. To prevent acid rain, coal plants are required by the US EPA to clean the sulfur dioxide from there emmissions using lime (CaO) according to the following reaction: CaO(s)+SO2(g)-->CaSO3(s) If a power plant emmits 10,000 L of SO2(g) in a day, how much lime will be needed in kilograms to clean their daily emissions? Assume standard temperature and pressure.

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Answer #1

At STP 1 mole of gas occupy volume 22.414 L then

10000 L SO2 = 10000/22.414 = 446.149 mole SO2

reaction is CaO(g) + SO2(g) CaSO3(s)

According to reaction CaO & SO2 react equimolar proportion thus, 446.149 mole of CaO require to complete reaction with SO2

molar mass of CaO = 56.0774g/mol that mean 1 mole of CaO = 56.0774g then 446.149 mole of CaO =

56.0774446.149 = 25018.87 gm of CaO require

25018.87 gm = 25.01887 Kg

25.01887 Kg of CaO require to clean daily emission.

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