H2
SO2
H2S
CO2
Explanation
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Discussions (13)
SO2 can act as both oxidizing as well as reducing agent since it has +4 oxidation state which is exactly between its highest oxidation state +6 and lowest oxidation state +2 ,Thus it can change its oxidation number either from +4 to-2(reduction) and +4 to+6 (oxidation) .
Where as in H2S the oxidation state of sulphur is -2 so it can lose electrons to attain +4 and +6 oxidation state but it can not gain the electrons. Therefore, H2S act as reducing agent only.
In new school chemistry... H2S only acts as a precipitating agent and reducing agent....
Check page 386, 387 and 388...
In the same textbook,,, SO2 acts as both oxidizing and reducing agent...
Check page 390 to 393...
I mean to write SO2....Though it acts as reducing agent in many of its reaction, it still plays the role of an oxidizing agent when treated with a more powerful reducing agent (e.g H2S)
Hydrogen acts as reducing agent as well as oxidising agent.It acts as reducing agent with non metals because it donates electron which will oxidise non metal. And as oxidising agent with etal by accepting the electrons.
and also In
S
O
2
, sulphur having oxidation state
+
4
so it can lose its two more electrons to attain
+
6
oxidation state. Therefore it can lose and gain electron therefore it acts as oxidising as well as reducing agent.
so both H2 and SO4 are correct.
Some compounds can act as either oxidizing agents or reducing agents. One example is hydrogen gas, which acts as an oxidizing agent when it combines with metals and as a reducing agent when it reacts with nonmetals.
H2 (gas) acts as both reducing and
oxidized agent...another example is Hydrogen peroxide..H2O2
