Emf & Electrode Potential NCERT Exercise Based MCQs Redox Reactions Chemistry NEET Practice Questions, MCQs, Past Year Questions (PYQs), NCERT Questions, Question Bank, Class 11 and Class 12 Questions, and PDF solved with answers

Q1:

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

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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

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Q3:

The ${Mn}^{3 +}$ ion is unstable in solution and undergoes disproportionation reaction to give ${Mn}^{2 +},$ ${MnO}_{2}$ $and$ $H^{+}$ ion. The balanced ionic equation for the reaction is-

1.	$\small{2 \mathrm{Mn}^{3+}{ }_{(\mathrm{aq})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow \mathrm{MnO}_{2(\mathrm{~s})}+\mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}}$
2.	Mn³⁺_(aq) + H₂O_(l) → MnO_2(s) + 2Mn²⁺_(aq) + 4H⁺_(aq)
3.	$\small{5 \mathrm{Mn}^{3+}(\mathrm{aq})+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow \mathrm{MnO}_{2(\mathrm{s})}+3 \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})}$
4.	$\small{2 \mathrm{Mn}^{3+}{ }_{(\mathrm{aq})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow 2 \mathrm{MnO}_{2(\mathrm{s})}+2 \mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}}$

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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

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

The negatively charged electrode will be-

1. Zn

2. Ag

3. Both

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.	\(\small{2 \mathrm{Mn}^{3+}{ }_{(\mathrm{aq})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow \mathrm{MnO}_{2(\mathrm{~s})}+\mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}}\)
2.	Mn³⁺_(aq) + H₂O_(l) → MnO_2(s) + 2Mn²⁺_(aq) + 4H⁺_(aq)
3.	\(\small{5 \mathrm{Mn}^{3+}(\mathrm{aq})+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow \mathrm{MnO}_{2(\mathrm{s})}+3 \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})}\)
4.	\(\small{2 \mathrm{Mn}^{3+}{ }_{(\mathrm{aq})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow 2 \mathrm{MnO}_{2(\mathrm{s})}+2 \mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}}\)

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