The correct statement about electrolysis of an aqueous solution of ${\mathrm{CuCl}}_2$ with Pt electrode is-

1.	Cu2+  ion reduced at the cathode;  Cl-  ion oxidized at the anode
2.	Cu2+  ion reduced at the anode;  Cl-  ion oxidized at the cathode
3.	Cu2+  ion reduced at the cathode;  H2O  ion oxidized at the anode
4.	H2O  ion reduced at the cathode;  Cl-  ion oxidized at the anode

The oxidizing agent and reducing agent in the given reaction are :

$3{\mathrm{N}}_2{\mathrm{H}}_{4\left(\mathrm{l}\right)}+4{\mathrm{ClO}}_{3\left(\mathrm{aq}\right)}^{-}\to$
$6{\mathrm{NO}}_{\left(\mathrm{g}\right)}+4{\mathrm{Cl}}_{\left(\mathrm{aq}\right)}^{-}+6{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}$

1. Oxidising agent = ${\mathrm{N}}_2{\mathrm{H}}_4$; Reducing agent = ${\mathrm{ClO}}_3^{-}$

2. Oxidising agent = ${\mathrm{ClO}}_3^{-}$; Reducing agent = ${\mathrm{N}}_2{\mathrm{H}}_4$

3. Oxidising agent = ${\mathrm{N}}_2{\mathrm{H}}_4$ ; Reducing agent = ${\mathrm{N}}_2{\mathrm{H}}_4$

4. Oxidising agent = ${\mathrm{ClO}}_3^{-}$ ; Reducing agent = ${\mathrm{ClO}}_3^{-}$

The oxidising agent and reducing agent in the given reaction are :

${}_{}$${\mathrm{Cl}}_2{\mathrm{O}}_{7\left(\mathrm{g}\right)}+4{\mathrm{H}}_2{\mathrm{O}}_{2\left(\mathrm{aq}\right)}+2{\mathrm{OH}}_{\left(\mathrm{aq}\right)}^{-}\to$
$2{\mathrm{ClO}}_{2\left(\mathrm{aq}\right)}^{-}+4{\mathrm{O}}_{2\left(\mathrm{g}\right)}+5{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}$${}_{}$

1. Oxidizing agent = H₂O₂; Reducing agent = ${\mathrm{Cl}}_2{\mathrm{O}}_7$

2. Oxidizing agent = ${\mathrm{Cl}}_2{\mathrm{O}}_7$; Reducing agent = ${\mathrm{H}}_2{\mathrm{O}}_2$

3. Oxidizing agent = H₂O₂; Reducing agent = H₂O₂

4. None of the above

Given a galvanic cell with the following reaction:

${\mathrm{Zn}}_{\left(\mathrm{s}\right) } + 2{{\mathrm{Ag}}^{+}}_{\left(\mathrm{aq}\right)} \to {{\mathrm{Zn}}^{+2}}_{\left(\mathrm{aq}\right)} + {\mathrm{2Ag}}_{\left(\mathrm{s}\right)}$

Which electrode will be negatively charged?

1. Zn

2. Ag

3. Both Zn and Ag

4. None of the above.

The oxidation states of the central atom in the given species are, respectively:

${\mathrm{H}}_4{\mathrm{P}}_2{\mathrm{O}}_7$ $$ $\mathrm{and}$ ${\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_7$

KI₃, H₂S₄O₆

The oxidation numbers of iodine and sulphur in the above compounds are, respectively:

1. \(\dfrac{1}{3}\) ; 4
2. 2.5 ; \(\dfrac{1}{3}\)
3. \(-\dfrac{1}{3}\) ; 2.5
4. 2.5 ; 3

The correct example of metal displacement reaction among the following is:

1. $\mathrm{Fe}+2\mathrm{HCl}\to {\mathrm{FeCl}}_2+{\mathrm{H}}_2\uparrow$

2. $2\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2\to 2\mathrm{PbO}+4{\mathrm{NO}}_2+{\mathrm{O}}_2\uparrow$

3. $2{\mathrm{KClO}}_3\stackrel{∆}{\to }2\mathrm{KCl}+3{\mathrm{O}}_2$

4. ${\mathrm{Cr}}_2{\mathrm{O}}_3+2\mathrm{Al}\stackrel{∆}{\to }{\mathrm{Al}}_2{\mathrm{O}}_3+2\mathrm{Cr}$

2 Na(s) + H₂(g) → 2 NaH (s)

The incorrect statement among the following regarding above mentioned reaction is:

1. Na gets oxidised
2. It is a redox reaction
3. NaH is an ionic hydride
4. None of the above

Consider the given reaction:
\(2 \mathrm{Cu}_2 \mathrm{O}(s)+\mathrm{Cu}_2 \mathrm{~S}(s) \rightarrow 6 \mathrm{Cu}(s)+\mathrm{SO}_2(g)\)

Which of the following statements about the given reaction is correct?
1. Cu is reduced and Cu(I) is an reductant.
2. Sulphur is reduced and S in Cu₂S acts as oxidant.
3. Cu(I) is an oxidant and Cu(I) is reduced.
4. Sulphur is reduced and copper is oxidised.

The species among the following that does not show a disproportionation reaction is-

ClO^–, ClO₂^–, \(ClO_{3}^{-}\) and ClO₄^–

1. ClO^–
2. ClO₂^–
3. ClO₄^–
4. \(ClO_{3}^{-}\)