The oxidation state of Cr in [Cr(NH₃)₄Cl₂]⁺ is [AIEEE 2005]

(1) +3

(2) +2

(3) +1

(4) 0

A brown ring complex compound is formulated as $\left[Fe{\left(H_{2}O\right)}_{5}NO\right]S{O}_4.$ The oxidation state of iron is 

1. 1

2. 2

3. 3

4. 0

The oxidation number of P in Mg₂P₂O₇ is - 

What is the oxidation number of sulphur in $N{a}_2{S}_4{O}_6$ - 

(1) $\frac{2}{3}$

(2) $\frac{3}{2}$

(3) $\frac{3}{5}$

(4) $\frac{5}{2}$

What is the oxidation number of Co in $\left[Co{\left(N{H}_3\right)}_{4}ClN{O}_2\right]$

(1) + 2

(2) + 3

(3) + 4

(4) + 5

When KMnO₄ acts as an oxidizing agent and ultimately forms \(\left[\mathrm{MnO}_4\right]^{-2}, \mathrm{MnO}_2, \mathrm{Mn}_2 \mathrm{O}_3, \mathrm{Mn}^{+2}\)${}^{}$
then the number of electrons transferred in each case, respectively, are:

For the redox reaction $Mn{O}_4^{-}+C_2{O}_4^{-2}+H^{+}\to M{n}^{2+}+C{O}_2+H_{2}O$ the correct coefficients of the reactants for the balanced reaction are 

Which of the following is the strongest oxidising agent?

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

If the chemical reaction given below is assumed to be balanced, what will be the values of a, b, c, and d, respectively?

$I{O}_3^{-}+a{I}^{-}+b{H}^{+}\to c{H}_{2}O+d{I}_2$

1. 5, 6, 3, 3 

2. 5, 3, 6, 3

3. 3, 5, 3, 6

4. 5, 6, 5, 5

The number of moles of KMnO₄ reduced by one mole of KI in an alkaline medium is:

1. One fifth

2. five

3. One

4. Two