Question 2 :
The equilibrium constant of the following redox reaction at $298\ K$ is $1\times 10^{8}$<br/><br/><div>$2Fe^{3+}(aq.) + 2I^{-}(aq.) \rightleftharpoons 2Fe^{2+}(aq.) + I_{2}(s)$<br/><br/><div>If the standard reduction potential of iodine becoming iodides is $+ 0.54\ V$. What is the standard reduction potential of $Fe^{3+}/ Fe^{2+}$?</div></div>

Question 3 :
Assertion: E$^{0}$ value of single electrode is determined experimentally by combining the electrode with SHE. Reason: SHE is taken as a reference electrode.

Question 5 :
A certain current liberated 0.504 gm of hydrogen in 2 hrs. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution?

Question 6 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">The potential across the metal and the aqueous solution of its ions of unit activity at 298K is known as:</p>

Question 8 :
$K, Ca$ and $Li$ metals may be arranged in the decreasing order of their standard electrode potentials as____________.

Question 9 :
A hydrogen gas. electron is made by dipping platinum wire in a solution of$HCI$ of $pH=10$ and by passing hydrogen gas around the platinum wire at one atm pressure.The oxidation potential of electrode would be ?

Question 12 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">For which of the following SOP and SRP are equal:</p>

Question 13 :
Which change could take place at the anode of an electro chemical cell?

Question 14 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">The standard hydrogen electrode has zero electrode potential because: </p>

Question 15 :
The standard ${E}_{red}^{o}$ values of $A, B$ and $C$ are $+0.68V, -2.54V, -0.50V$ respectively. The order of their reducing power is:

Question 17 :
$E^o$ value of $Ni^{2+}/Ni$ is $-0.25$V and $Ag^+/Ag$ is $+0.80$V. If a cell is made by taking the two electrodes what is the feasibility of the reaction?

Question 18 :
<div>Calculate $E^{\circ}$ values of the following reactions.<br/></div> $2Ag + Zn^{2+} \rightarrow 2Ag^+ + Zn$<div><br/></div><div>Given that: $E^{\circ}_{Ag^{+}/Ag}=0.80 V, E^{\circ}_{Zn^{2+}/Zn}=-0.76 V$</div>

Question 19 :
The standard electrode potential of $Cu | Cu^{+2} $ is $ - 0.34 $ Volt. At what concentration of $Cu^{+2} $ ions, electrode potential will be zero?

Question 20 :
Assertion: The absolute value of the electrode potential cannot be determined experimentally Reason: The electrode potentials are generally determined with respect to standard hydrogen electrodes.<br/>

Question 21 :
The oxidation potential of hydrogen electrode at pH = 10 and P$_{H_2}$ = 1 atm is __________.

Question 24 :
The standard reduction potential for $Cu^{2+}/Cu$ is $+0.34$V. What will be the reduction potential at pH$=14$? [Given: $K_{sp}$ of $Cu(OH)_2$ is $1.0\times 10^{-19}]$.

Question 25 :
Aluminum displaces hydrogen in dil. HCl whereas silver does not. The e.m.f of a cell prepared by combination $Al/{ Al }^{ 3+ }\ and\ Ag/{ Ag }^{ + }$ is 2.46 V. The reduction potential reduction potential of aluminum electrodes is:<br/>

Question 26 :
Aluminium displaces hydrogen from dilute $ \mathrm{HCl} $ whereas silver does not. The E.M.F. of the cell prepared by combining $ \mathrm{A} / \mathrm{Al}^{3+} $ and $ \mathrm{Ag} / \mathrm{Ag}^{+} $ is $ 2 \cdot 46 \mathrm{V} $. The reduction potential of silver electrode is $ +0.80 \mathrm{V} $. The reduction potential of aluminium electrode is

Question 27 :
Which of the following is/are correct? Given, the half-cell emf is {tex} \mathrm E _ { \mathrm { Cu } ^ { 2 + } / \mathrm { cu } } ^ { \circ } = 0.337 , \mathrm E _ { \mathrm { Cu } ^ { + } / \mathrm { cu } } ^ { \circ } = 0.521 {/tex}

Question 28 :
<div>State True or False.<br/></div>The absolute value of standard single electrode potential can be determined experimentally.

Question 29 :
For the cell {tex} \mathrm { Tl } \left| \mathrm { Tl } ^ { + } ( 0.001 \mathrm { M } ) \| \mathrm { Cu } ^ { 2 + } ( 0.1 \mathrm { M } ) \right| \mathrm { Cu } .\ \mathrm E _ { \mathrm { cell } } ^ { \circ } {/tex} at {tex} 25 ^ { \circ } \mathrm { C } {/tex} is {tex} 0.83 \mathrm { V } , {/tex} which can be increased:

Question 30 :
Assertion: If standard reduction potential for the reaction, $Ag^{+} + e^{-}\rightarrow Ag$ is $0.80\ volt$, then for the reaction, $2Ag^{+} + 2e^{-}\rightarrow 2Ag$, it will be $1.60\ volt$. Reason: If concentration of $Ag^{+}$ ions is doubled, the electrode potential is also doubled.

Question 31 :
Given:<br> {tex} \mathrm { A } ^ { 2 + } + 2 \mathrm e ^ { - } \rightarrow \mathrm { A } ( \mathrm { s } ) \quad \mathrm E ^ { \ominus } = 0.8 \mathrm { V } {/tex} <br>{tex} \mathrm { B } ^ { \oplus } + \mathrm e ^ { - } \rightarrow \mathrm { B } ( \mathrm { s } ) \quad \mathrm E ^ { \ominus } = - 0.64 \mathrm { V } {/tex}<br> {tex} \mathrm { X } _ { 2 } ( \mathrm { g } ) + 2 \mathrm e ^ { - } \rightarrow 2 \mathrm { X } ^ { \ominus } \quad \mathrm E ^ { \ominus } = 1.03 \mathrm { V } {/tex}<br> Which of the following statements is/are correct?

Question 32 :
Assertion: Emf and potential difference are same for cell. Reason: Both gives the difference in electrode potential under any condition.

Question 33 :
If $Cu$ reacts with conc. $H_2SO_4$, then what reactions take place:

Question 34 :
For the cell prepared from electrode A and B, electrode A : $\dfrac { { Cr }_{ 2 }{ O }_{ 7 }^{ 2- } }{ { Cr }^{ 3+ } } $, ${ E }_{ red }^{ 0 }$ = +1.33 V and electrode B : $\dfrac { {Fe}^{ 3+ } }{ { Fe }^{2+}}$ , ${ E }_{ red }^{ 0 }$ = 0.77 V, which of the following statement is not correct ?

Question 36 :
<p> <font face="Cambria Math, serif">Among Na, Hg, S, Pt, and graphite which can be used as electrode in electrolytic cell having aqueous solutions?</font></p>

Question 37 :
Consider the equilibrium obtained by electrically connecting zinc- amalgam $Zn (Hg)$ and $HgO$ electrodes in mercury cell,<br/><br/><div>$Zn (Hg) + HgO(s) \displaystyle \rightleftharpoons ZnO(s) + Hg(l)$<br/><br/></div><div>Under this equilibrium, what is the relation between the potential of the $Zn (Hg)$ and $HgO$ electrodes measured against the standard hydrogen electrode?</div>

Question 38 :
<p> <font face="Cambria Math, serif">Which of the following statements is /are correct?</font></p>

Question 39 :
<b><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span></b><p class="wysiwyg-text-align-left">List I List II</p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">A) Salt bridge 1) Reduction</p><p class="wysiwyg-text-align-left">B) Standard hydrogen electrode 2) Oxidation</p><p class="wysiwyg-text-align-left">C) Cathode 3) Reference electrode<br/></p><p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"> D) Anode 4) KCl,KNO$_{3},$</span></span></p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"> (or) NH$_{4}$NO$_{3}.$</span></span><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">.</span></span></p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">The correct match is :</p>

Question 40 :
<p> <font face="Cambria Math, serif">What weight of copper will be deposited by passing 2 faradays of electricity through a cupric salt (atomic weight of </font> <img style='object-fit:contain' align="absmiddle" src="https://storage.googleapis.com/teachmint/question_assets/JEE%20Advanced/60007ed7c4cbb406e88033c5"/> <font face="Cambria Math, serif">)?</font></p>

Question 41 :
<p align="justify"> <font face="Cambria Math, serif">In electrolysis of very dilute </font> <img style='object-fit:contain' align="absmiddle" src="https://storage.googleapis.com/teachmint/question_assets/JEE%20Advanced/6000913e5441933baf263d87"/> <font face="Cambria Math, serif"> solution, using platinum electrodes.</font></p>