Consider the standard electrode potentials given below:

(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)	\(E_{Cr^{3+}/Cr}^o = -0.74\ V\)

The correct arrangement of increasing order for 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

What is the oxidation state of phosphorus in the phosphate ion, PO₄³⁻?

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.

Which of the following hydrohalic acids acts as the best reducing agent?
1. HCl
2. HBr
3. HI
4. HF$\mathrm{}$

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