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:

1.	4, 3, 1, 5	2.	1, 5, 3, 7
3.	1, 3, 4, 5	4.	3, 5, 7, 1

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

In the equation

$H_{2}S+2HN{O}_3\to 2H_{2}O+2N{O}_2+S$

The equivalent weight of hydrogen sulphide is [BVP 2003]

(1) 16

(2) 68

(3) 34

(4) 17

If 1.2 g of metal displace 1.12 litre hydrogen at normal temperature and pressure, equivalent weight of metal would be 

(1) 24

(2) 12

(3) 1.2 $÷$ 11.2

(4) 1.2 $\times$ 11.2

The equivalent weight of phosphoric acid (H₃PO₄) in the reaction $NaOH+H_{3}P{O}_4\to Na{H}_{2}P{O}_4+H_{2}O$ is

(1) 25

(2) 49

(3) 59

(4) 98

What is the equivalent mass of $I{O}_4^{-}$ when it is converted into I₂ in acid medium

(1) M/6

(2) M/7

(3) M/5

(4) M/4

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?