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nid404:
product would be metal hydroxide and hydrogen

not always if the metal in the alkali is more reactive, there will be no reaction

holtadit:
Three reactions used in the manufacture of sulphuric acid are shown.

 S + O2 -> SO2

 2SO2 + O2 -> 2SO3

 SO3 + H2O -> H2SO4

Which of these reactions are redox reactions?

I dont understand how it is 1 and 2 only. Where is the reduction and oxidation going on each equation ?

Amr Fouad:

--- Quote from: Ari Ben Canaan on April 10, 2010, 07:00:33 am ---Three reactions used in the manufacture of sulphuric acid are shown.

 S + O2 -> SO2

 2SO2 + O2 -> 2SO3

 SO3 + H2O -> H2SO4

Which of these reactions are redox reactions?

I dont understand how it is 1 and 2 only. Where is the reduction and oxidation going on each equation ?

--- End quote ---

Alright..here's the deal..First and foremost, you have to calculate the oxidation state of the Sulpher species..

1) It goes from 0 in Sulpher (natural element) to +4 i sulpher dioxide...
SO^2...X+(2x-2)=0
and so X=+4.....sulpher is oxidzed

2) It goes from +4 in sulpher dioxide (again) to +6 in sulpher trioxide..
SO^3...X+(-2x3)=0
X=+6..sulpher is oxididzed again

3) No redox reaction
It goes from +6 in sulpher trioxide to +6 in sulphuric acid...
H^2SO^4.....
The H ion is +1..and since there are 2 such ions...the sulphate ion SO^4 must have a charge of -2..

X+(4x-2)=-2
X=+6

Hope that helped..

holtadit:
Excellent explanation. I completely understood.


+rep :)

nid404:
thanks amr

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