Question

PLEASE HELP!

Sulfur dioxide emissions from flue gases at 95 ° C can be removed by a commercial process involving the following reactions:
SO2 + Cl2 ---> SO2Cl2
SO2Cl2 + 2H2O ---> H2SO4 + 2HCl
H2SO4 + Ca (OH)2 ---> CaSO4 + 2H2O
Assuming 95.0% process efficiency, how many grams of calcium sulfate do we get from 100 grams of sulfur dioxide?

Answer 1

49.54 g

Step-by-step explanation:

Let's take the masses of both calcium sulfate and sulfur dioxide formed.

Sulfur dioxide = 32 + 2(16) = 64 g

Calcium sulfate = 40 + 32 + 4(16) = 136 g

So, under ideal conditions, to produce 136 g of Calcium sulfate, we require 64 g of Sulfur dioxide.

But, it mentions the process is only 95% efficient.

Hence, taking the ratio :

`(64)/(136) = (0.95x)/(100)`

`0.95x = (64 * 100)/(136)`

`0.95x = (6400)/(136)`

`x = (800)/(17) * (20)/(19)`

`x = (16000)/(323)`

x = 49.54 g (approximately)