One commercial system removes `SO_(2)` emission from smoke at `95(@)C` by the following set of reaction :
`SO_(2)(g)+Cl_(2)(g) to SO_(2)Cl_(2)`(g)
`SO_(2)Cl_(2)(g) +H_(2)O(l) to H_(2)SO_(4)+HCl`
`H_(2)SO_(4)+Ca(OH)_(2) to CaSO_(4)+H_(2)O`
How many grams of `CaSO_(4)` may be produced from 3.78 g of `SO_(2)` ?

One commercial system removes SO_(2) emmission from smoke at 95^(@) C by the following set of reactions- SO_(2)(g)+ Cl_(2)(g) to SO_(2)Cl_(2)(g) SO_(2)Cl_(2) + 2H_(2)O to H_(2)SO_(4) + 2HCl H_(2)SO_(4) + Ca(OH)_(2) to CaSO_(4) + 2H_(2)O Assuming the process to be 95% efficient . How many moles of CaSO_(4) may be produced from 128 g SO_(2).[Ca=40,S-32,O-16]

underline(S)O_(2)Cl_(2)+H_(2)O to H_(2)SO_(4)+HCl

underline(S)O_(2)Cl_(2)+H_(2)O to H_(2)SO_(4)+HCl

Ca(OH)_(2)+SO_(2) to CaSO_(3)darr+H_(2)O

Ca(OH)_(2)+SO_(2) to CaSO_(3)darr+H_(2)O

Ca(OH)_(2)+SO_(2) to CaSO_(3)darr+H_(2)O

How many grams of H_(2)SO_(4) are present in 0.25 g mole of H_(2)SO_(4) ?