\[{{H}_{2}}S\] acts only as a reducing agent while \[S{{O}_{2}}\]can act both as a reducing and oxidizing agent because [AMU 1999]

\[S\]in \[S{{O}_{2}}\]has oxidation state + 4

\[S\]in \[{{H}_{2}}S\]has - 2 oxidation state

Hydrogen in \[{{H}_{2}}S\]more +ve than oxygen

Oxygen is more - ve in \[S{{O}_{2}}\]

\[{{H}_{2}}S\] acts only as a reducing agent while \[S{{O}_{2}}\]can a

1.	\[{{H}_{2}}S\] acts only as a reducing agent while \[S{{O}_{2}}\]can act both as a reducing and oxidizing agent because [AMU 1999]
A.	\[S\]in \[{{H}_{2}}S\]has - 2 oxidation state
B.	\[S\]in \[S{{O}_{2}}\]has oxidation state + 4
C.	Hydrogen in \[{{H}_{2}}S\]more +ve than oxygen
D.	Oxygen is more - ve in \[S{{O}_{2}}\]
Answer» B. \[S\]in \[S{{O}_{2}}\]has oxidation state + 4

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\[{{H}_{2}}S\] acts only as a reducing agent while \[S{{O}_{2}}\]can act both as a reducing and oxidizing agent because [AMU 1999]

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