Redox Reactions...

Consider the following out of $$\underset { \left( I \right)  }{ H_{ 2 }SO_{ 4 } } \underset { \left( II \right)  }{ ,H_{ 2 }S_{ 2 }O_{ 8 }, } { \underset{III}{H_{ 2 }SO_{ 5 }},\underset{IV}{H_{ 2 }S_{ 2 }O_{ 3 } }} $$ and $$\underset { \left( V \right)  }{ { H }_{ 2 }{ S }_{ 2 }{ O }_{ 7 } } $$
Choose the correct option.

Which of the following show non-zero multiple oxidation state?

Sugarcane on reaction with nitric acid gives?

Which of the following pairs of elements show similar set of oxidation state?

Four $$Cl_{2}$$ molecules undergo a loss and gain of $$6$$ mole of electrons to form two oxidation states of $$Cl$$ in auto redox change. What are the $$+ve$$ and $$-ve$$ oxidation states of $$Cl$$ in the change:

The $$O.S.$$ of $$Fe$$ in $$Na_{2}[Fe(CN)_{5}NO]$$ and $$Na_{4}[Fe(CN)_{5}NOS]$$ is:

A solution contains $${Fe}^{+2},{Fe}^{+3}$$ and $${I}^{-}$$ ions. This solution was treated with iodine at $${35}^{o}C$$. Then the favourable redox reaction is: 

Given reaction $$HCHO \rightarrow CH_{3}OH+HCOO^{-}$$ is an example of:

In the following structure, the oxidation number on carbon will be: $$H-N=C$$:-

How many electrons should $${ X }_{ 2 }{ H }_{ 4 }$$ liberate so that in the new compound X shows oxidation number of -1/2? $$\left( E,N.X>H \right) $$