The strongest oxidising agent among the following is -

1. $Br{O}_3^{-}/B{r}^{2+},E^o=+1.50$

2. $F{e}^{3+}/F{e}^{2+},E^o=+0.76$

3. $Mn{O}_4^{-}/M{n}^{2+},E^o=+1.52$

4. $C{r}_2{O}_7^{2-}/C{r}^{3+},E^o=+1.33$

In an alkaline medium ClO₂ oxidize H₂O₂ in O₂ and reduces itself in Cl^– . How many moles of H₂O₂ will be oxidized by one mole of ClO₂?

Oxidation number of oxygen in potassium super oxide (KO₂) is-

1. – 2

2. – 1

3. – 1/2

4. – 1/4

The oxidation state of Cu in  ${\mathrm{YBa}}_2{\mathrm{Cu}}_3{\mathrm{O}}_7$  is -

(Yttrium = +3)

The oxidation number of P in Mg₂P₂O₇ is - 

The oxidation number of S in H₂S₂O₈ is:

1. + 2

2. + 4

3. + 6

4. + 7

Sn⁺⁺ loses two electrons in a reaction. The final oxidation number of tin will be-

1. + 2

2. Zero

3. + 4

4. – 2

The number of moles of MnO^-₄ required to oxidise one mole of ferrous oxalate completely in an acidic medium is-

1. 0.6 mole

2. 0.4 mole

3. 7.5 moles

4. 0.2 mole

The oxidation states of P in H₄P₂O₅, H₄P₂O₆, H₄P₂O₇, are respectively -

If 10 gm of V₂O₅ is dissolved in acid and is reduced to V²⁺ by zinc metal, how many moles of I₂ could be reduced by the resulting solution if it is further oxidized to VO²⁺ ions?

[Assume no change in state of Zn²⁺ions] (V = 51, O =16, I = 127) :