(a)	\(E_{k^+/K}^o = - 2.93\ V\); \(E_{Ag^+/Ag}^o = 0.80\ V\)
(b)	\(E_{Hg^{2+}/Hg}^o = 0.79\ V\); \(E_{Mg^{2+}/Mg}^o = - 2.37\ V\)
(c)	\(E_{Cr^{3+}/Cr}^o = -0.74\ V\)

Based on standard electrode potentials given above, the correct arrangement for increasing order of reducing power of
elements is: 

1.	\(\mathrm{Ag}<\mathrm{Hg}<\mathrm{Cr}<\mathrm{Mg}<\mathrm{K} \)
2.	\(\mathrm{Ag}>\mathrm{Cr}>\mathrm{Mg}>\mathrm{Hg}>\mathrm{K}\)
3.	\(\mathrm{K}>\mathrm{Mg}<\mathrm{Cr}<\mathrm{Hg}>\mathrm{Ag} \)
4.	\(\mathrm{K}<\mathrm{Mg}<\mathrm{Cr}<\mathrm{Hg}<\mathrm{Ag}\)

The oxidation state of two S-atoms in ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ is:

1. +2 and +4

2. +3 and -2

3. +4 and -2

4. +6 and -2

the oxidation state of P in ${\mathrm{PO}}_4^{3-}$?

1. +2

2. +3

3. +4

4. +5

The oxidation state of P in ${\mathrm{HPO}}_3^{2-}$ is-

Nitric acid reacts with PbO but does not react with PbO₂ , because -

1. PbO is a base while PbO₂ is a strong oxidizing reagent

2. PbO is a base while PbO₂ is a weak oxidizing reagent

3. PbO is neutral while PbO₂ is a strong oxidizing reagent

4. PbO is acid while PbO₂ is a strong oxidizing reagent

In the given reaction, what is the name of the species that bleaches the substances due to its oxidising action?

Cl₂(g) + 2OH^-(aq) → ClO^-(aq) + Cl^-(aq) + H₂O(l)

1. ClO^- 

2. Cl₂

3. Cl^-

4. Both ClO^- and Cl^-

The compound AgF₂ (unstable) acts as a/ an:

1. Oxidising agent.

2. Reducing agent.

3. Both oxidising and reducing agent.

4. Neither oxidising and reducing agent.

Among the following hydrohalic compounds, the best reductant is -

$1. \mathrm{HCl}$
$2. \mathrm{HBr}$
$3. \mathrm{HI}$
$4. \mathrm{HF}$

KMnO₄ (mol. wt=158) oxidizes oxalic acid in acidic medium to CO₂ and water as follows.

$5{\mathrm{C}}_2{\mathrm{O}}_4^{2-}+2{\mathrm{MnO}}_4^{-}+16{\mathrm{H}}^{+}\to 10{\mathrm{CO}}_2+2{\mathrm{Mn}}^{2+}+8{\mathrm{H}}_2\mathrm{O}$

What is the equivalent weight of KMnO₄?

1. 158

2. 31.6

3. 39.5

4. 79