Use oxidation numbers to identify if this reaction is REDOX reactions.
SO2(g) + H2O(l) -> H2SO3(aq)
for oxidation #s I got:
SO2 = -2 for the S
= -2 for the o2
H20 = +1 for H2
= -2 for O
-->
H2SO = +1 for H2
= -2 for S
= -2 for O3
There for one oxygen was reduced hence REDOX did occure
True??
To determine if a reaction is a redox reaction, you need to compare the oxidation numbers of the reactants and products. In a redox reaction, there should be a change in the oxidation number of at least one element.
Let's calculate the oxidation numbers for the elements in the given reaction:
In SO2:
The oxygen atoms in SO2 usually have an oxidation number of -2 each, so the total oxidation number for the oxygen atoms is -4.
Since the overall charge of the molecule is neutral, the oxidation number of sulfur (S) must be +4 in order to balance out the -4 from the oxygen.
In H2O:
Hydrogen (H) typically has an oxidation number of +1.
The oxygen atom usually has an oxidation number of -2.
Since water is neutral, the sum of the oxidation numbers should be zero.
Therefore, the oxidation number of O in H2O is -2.
In H2SO3:
Hydrogen (H) typically has an oxidation number of +1.
Again, the oxygen atom usually has an oxidation number of -2.
To find the oxidation number of sulfur (S), we assume it to be x.
So, 2(1) + x + 3(-2) = 0
2 + x - 6 = 0
x - 4 = 0
x = +4
From the calculation, the oxidation number of sulfur in SO2 changes from +4 to +2, meaning it is reduced. Since there is a change in the oxidation number of an element (in this case, sulfur), the given reaction is indeed a redox reaction.
So, your conclusion that redox occurred in the reaction is correct.