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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.	$\mathrm{K}<\mathrm{Mg}<\mathrm{Cr}<\mathrm{Hg}<\mathrm{Ag}$

Subtopic: Emf & Electrode Potential |

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Q2:

The correct statement about the given reaction is-

(CN)_2(g) + 2OH^-_(aq) $\to$ CN^-_(aq) + CNO^-_(aq) + H₂O_(l)

1.	The reaction is an example of a disproportionation reaction.
2.	Hydrogen atom gets oxidized.
3.	Reaction occurs in acidic medium.
4.	None of the above

Subtopic: Emf & Electrode Potential |

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Q3:

The Mn³⁺ ion is unstable in solution and undergoes disproportionation reaction to give Mn²⁺, MnO₂ and H⁺ ion. The balanced ionic equation for the reaction is-

1.	$2 \mathrm{Mn}^{3+}{ }_{(\mathrm{aq})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$→${\mathrm{MnO}_{2(\mathrm{~s})}+\mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}}$
2.	$ \mathrm{Mn^{3+}_{(aq)} + H_2O_{(l)} } $ → ${\mathrm{MnO}_{2(\mathrm{~s})}+\mathrm{2Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}}$
3.	$5 \mathrm{Mn}^{3+}(\mathrm{aq})+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$→$\mathrm{MnO}_{2(\mathrm{s})}+3 \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})$
4.	$2 \mathrm{Mn}^{3+}{ }_{(\mathrm{aq})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} $→$2 \mathrm{MnO}_{2(\mathrm{s})}+2 \mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}$

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Q4:

The correct statement about the electrolysis of an aqueous solution of ${AgNO}_{3}$ with Pt electrode is:

1.	Pt(s) gets oxidized at cathode whereas Ag + ( aq ) gets reduced at anode
2.	Ag⁺ (aq) gets reduced at cathode and is oxidized at anode
3.	Ag⁺ (aq) gets reduced at cathode whereas water is oxidized at anode
4.	Ag (s) gets oxidized at cathode whereas H₂O is oxidised at anode

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Q5:

The correct statement about electrolysis of an aqueous solution of ${CuCl}_{2}$ 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

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Q6:

Given a galvanic cell with the following reaction:

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

Which electrode will be negatively charged?

1. Zn

2. Ag

3. Both Zn and Ag

4. None of the above.

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

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.	\(\mathrm{K}<\mathrm{Mg}<\mathrm{Cr}<\mathrm{Hg}<\mathrm{Ag}\)

1.	\(2 \mathrm{Mn}^{3+}{ }_{(\mathrm{aq})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}\)→\({\mathrm{MnO}_{2(\mathrm{~s})}+\mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}}\)
2.	\( \mathrm{Mn^{3+}_{(aq)} + H_2O_{(l)} } \) → \({\mathrm{MnO}_{2(\mathrm{~s})}+\mathrm{2Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}}\)
3.	\(5 \mathrm{Mn}^{3+}(\mathrm{aq})+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}\)→\(\mathrm{MnO}_{2(\mathrm{s})}+3 \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})\)
4.	\(2 \mathrm{Mn}^{3+}{ }_{(\mathrm{aq})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \)→\(2 \mathrm{MnO}_{2(\mathrm{s})}+2 \mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}\)

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