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Q1:

Which of the following electrodes will act as anodes, when connected to Standard Hydrogen Electrode?
$\begin{array}{rlr}\text { (a) } & \mathrm{{Al}^{3+} / {Al}} & \mathrm{{E}_{RP}^{o}=-1.66} \\\text { (b) } & \mathrm{{Fe}^{2+} / {Fe}} & \mathrm{{E}_{RP}^{o}=-0.44} \\\text { (c) } & \mathrm{{Cu}^{2+} / {Cu}} & \mathrm{{E}_{RP}^{o}=+0.34} \\\text { (d) } & \mathrm{{F}_{2}({~g}) / 2 {~F}^{-}({aq})} & \mathrm{{E}_{RP}^{o}=+2.87}\end{array}$

The correct choice among the above is:

1. (a, b)

2. (b, c)

3. (c, d)

4. (a, d)

Subtopic: Emf & Electrode Potential |

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Q2:

The reducing ability of the metals K, Au, Zn, and Pb follows the order

1.	K > Pb > Au > Zn	2.	Pb > K > Zn > Au
3.	Zn > Au > K > Pb	4.	K > Zn > Pb > Au

Subtopic: Application of Electrode Potential | Emf & Electrode Potential |

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Q3:

$E^{Θ}$ values of some redox couples are given below. On the basis of these values choose the correct option.

$E^{Θ} values : {Br}_{2} / {Br}^{-} = + 1.90$
${Ag}^{+} / Ag (s) = + 0.80$
${Cu}^{2 +} / Cu (s) = + 0.34;$
$I_{2} (s) / I^{-} = + 0.54$

1.	Cu will reduce Br^–	2.	Cu will reduce Ag
3.	Cu will reduce I^–	4.	Cu will reduce Br₂

Subtopic: Emf & Electrode Potential |

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Q4:

Given below are two statements:

Assertion (A):	Among halogens, fluorine is the best oxidant.
Reason (R):	Fluorine is the most electronegative atom.

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	(A) is False but (R) is True.

Subtopic: Emf & Electrode Potential |

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Q5:

Under standard conditions ,the reactions that is/are spontaneous:

Half-Reaction	Eº(V)
Cu⁺(aq) + e¯ → Cu(s)	+0.52
Co²⁺(aq) + 2 e¯ → Co(s)	–0.28
In³⁺(aq) + 3 e¯ → In(s)	–0.34

I. 2 Cu⁺(aq) + Co(s) → Co²⁺(aq) + 2 Cu(s)
II. 3 Co²⁺(aq) + 2 In(s) → 2 In³⁺(aq) + 3 Co(s)

1.	I only	2.	II only
3.	Both I and II	4.	Neither I nor II

Subtopic: Emf & Electrode Potential |

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Level 2: 60%+

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Hints

Please attempt this question first.

Q6:

At $298 {~K},$ the standard electrode potentials of $\mathrm{{Cu}^{2+} /{Cu},}$ $\mathrm{{Zn}^{2+} / {Zn},~~ {Fe}^{2+} / {Fe}}$ and $\mathrm{{Ag}^{+} / {Ag}} $ are $\mathrm{0.34 {~V}, -0.76 {~V},}$ $\mathrm{-0.44 {~V}}$ and $\mathrm{0.80 {~V},}$ respectively.
On the basis of standard electrode potentials, predict which of the following reaction can not occur?

1.	$\mathrm{2 {CuSO}_{4}({aq})+2 {Ag}({s}) → 2 {Cu}({s})+{Ag}_{2} {SO}_{4}({aq})} $
2.	$\mathrm{{CuSO}_{4}({aq})+{Zn}({s})} $ $\mathrm{→ {ZnSO}_{4}({aq})+{Cu}({s})} $
3.	$\mathrm{{CuSO}_{4}({aq})+{Fe}({s})} $ $\mathrm{→ {FeSO}_{4}({aq})+{Cu}({s})} $
4.	$\mathrm{{FeSO}_{4}({aq})+{Zn}({s})} $ $→ \mathrm{{ZnSO}_{4}({aq})+{Fe}({s})} $

Subtopic: Emf & Electrode Potential |

69%

Level 2: 60%+

NEET - 2022

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Q7:

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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Q8:

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})} $→$2 \mathrm{MnO}_{2(\mathrm{s})}+2 \mathrm{Mn}^{2+}{ }_{(\mathrm{aq})}+4 \mathrm{H}^{+}{ }_{(\mathrm{aq})}$

Subtopic: Emf & Electrode Potential |

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Q9:

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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Q10:

The standard electrode potential (E°) values of Al³⁺/ Al, Ag⁺ / Ag, K⁺ / K, and Cr³⁺ / Cr are –1.66 V, 0.80 V, –2.93 V, & –0.79 V respectively. The correct decreasing order of the reducing power of the metals is:

1.	Ag > Cr > Al > K	2.	K > Al > Cr > Ag
3.	K > Al > Ag > Cr	4.	Al > K > Ag > Cr

Subtopic: Emf & Electrode Potential |

73%

Level 2: 60%+

NEET - 2019

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1.	\(\mathrm{2 {CuSO}_{4}({aq})+2 {Ag}({s}) → 2 {Cu}({s})+{Ag}_{2} {SO}_{4}({aq})} \)
2.	\(\mathrm{{CuSO}_{4}({aq})+{Zn}({s})} \) \(\mathrm{→ {ZnSO}_{4}({aq})+{Cu}({s})} \)
3.	\(\mathrm{{CuSO}_{4}({aq})+{Fe}({s})} \) \(\mathrm{→ {FeSO}_{4}({aq})+{Cu}({s})} \)
4.	\(\mathrm{{FeSO}_{4}({aq})+{Zn}({s})} \) \(→ \mathrm{{ZnSO}_{4}({aq})+{Fe}({s})} \)

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

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

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