Question 1 : <div>Assertion: The more negative is the standard reduction potential, greater is its ability to displace H$_2$ from acid.</div><div>Reason: Strength of reducing agent increases with the increase in the negative value of the standard reduction potential.<br/></div>

Question 2 : <div>Assertion: At the anode, the species having minimum reduction potential is formed by the oxidation of corresponding oxidizable species.</div><div>Reason: Species with minimum reduction potential has the highest tendency to get oxidized.<br/></div>

Question 3 : Which one is correct about a hypothetical electrochemical cell shown below?<br/>$\underset{A}{\ominus } | A^+ (XM) || B^+ (YM) |&#160;\underset{B}{\oplus} &#160; &#160; &#160; &#160; &#160; E_{cell} &#160;= + 0.20 V$<br/>

Question 4 : A gas $X$ at $1\ atm$ is bubbled through a solution containing a mixture of $1\ M\ Y^{-}$ and $1\ M\ Z^{-}$ at $25^{o}C.$ If the reduction potential of $Z &gt; Y &gt; X,$ then

Question 5 : The standard reduction potentials of ${ Cu }^{ 2+ }/Cu$ and ${ Cu }^{ 2+ }/{ Cu }^{ + }$ are $0.337$ and $0.153$V respectively. The standard&#160; electrode potential of ${ Cu }^{ + }/Cu$ half cell is:<br/>

Question 6 : The emf of the cell involving the following reaction, $\displaystyle { 2Ag }^{ + }+{ H }_{ 2 }\longrightarrow 2Ag+{ 2H }^{ + }$is $0.80$ volt. The standard oxidation potential of silver electrode is:

Question 7 : $E_{Cu^{2+}|Cu}^0 = + 0.337V, E_{Zn^{2+}|Zn}^0 = -0.762 V$.&#160;<br/><div>The EMF of the cell, $Zn | Zn^{2+} (0.1 M) || Cu^{2+} (0.01 M) | Cu$ is:</div>

Question 8 : The standard reduction potential values of three metallic cations of $X,\ Y$ and $Z$ are $0.52,\ -3.03$ and $-1.18\ V$ respectively. The order of reducing power of the corresponding metals is

Question 9 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">In an electro chemical process, a salt bridge is used</p><p class="wysiwyg-text-align-left">a) to maintain electro neutrality in each solution.</p><p class="wysiwyg-text-align-left">b) to complete the circuit so that current can flow</p><p>c) as an oxidising agent</p><p>d) as a colour indicator</p></span></span>

Question 12 : What will be standard cell potential of galvanic cell with the following reaction?<br>$2Cr_{(s)}+3Cd^{2+}_{(aq)}\rightarrow 2Cr^{3+}_{(aq)}+3Cd_{(s)}$<br>[Given: $E^o_{Cr^{3+}/Cr}=-0.74$V and $E^o_{Cd^{2+}/Cd}=-0.40$V]<br>

Question 13 : The efficiency of an hypothetical cell is about 84% which involves the following reaction :<br/>$A(s) \,+\, B^{2+} (aq) \rightarrow A^{2+} (aq) \,+\, B(s) \,:\, \Delta H \,=\, - 285 kJ$<br/>Then, the standard electrode potential of the cell will be: (Assume as $\displaystyle \Delta S \,=\, 0$)

Question 14 : Assertion: The reference electrode of silver-silver chloride is used as secondary reference electrode. Reason: The electrode is reversible with respect to Cl$^-$ ions.

Question 15 : It has been found experimentally that if standard reduction potential of oxidant - standard reduction potential of reductant is more than $1.7 V$ then their combination lead to explosion though it may be prevented by kinetic factors.<br/><br/><div>Now go through the following data and answer the questions.<br/>${ E }_{ { { Ag }^{ + } }/{ Ag } }^{ 0 }=0.80V$<br/>${ E }_{ { { ClO }_{ 4 }^{ - } }/{ { ClO }_{ 3 }^{ - } } }^{ 0 }=1.23V$<br/>${ E }_{ { { Fe }^{ 3+ } }/{ { Fe }^{ 2+ } } }^{ 0 }=0.77V$<br/>${ E }_{ { { MnO }_{ 4 }^{ - } }/{ { Mn }^{ 3+ } } }^{ 0 }=1.54V$<br/>${ E }_{ { { N }_{ 2 } }/{ { N }_{ 3 }^{ - } } }^{ 0 }=-3.09V$<br/>${ E }_{ { { Na }^{ + } }/{ Na } }^{ 0 }=-2.17V$<br/>${ E }_{ { { O }_{ 2 } }/{ { H }_{ 2 }{ O }_{ 2 } } }^{ 0 }=-1.03V$<br/><br/></div><div>Which of the following ionic combinations may lead to the formation of explosive substance?</div>

Question 16 : <p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">The standard electrode potential of Cu/Cu$^{+2}$ electrode is 0.336. It corresponds to the reaction:</span></span></p>

Question 17 : The chemical reaction taking place at the anode of a cell is

Question 18 : 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 standard electrode potential is also doubled.

Question 19 : Consider the cell<br/>$Pb(s)+{Hg}_{2}^{2+}(aq)\rightleftharpoons {Pb}^{2+}+Hg(l)$ voltage of the cell can be increased by?

Question 20 : If the following half cells have the ${E}^{o}$ values as<br>${ Fe }^{ 3+ }+e\rightarrow { Fe }^{ 2+ };{ E }^{ o }=+0.77V$ and ${ Fe }^{ 2+ }+2e\rightarrow Fe;{ E }^{ o }=-0.44V$; the ${E}^{o}$ of the half cell ${ Fe }^{ 3+ }+e\rightarrow Fe$ will be

Question 21 : The standard reduction potentials $E^{\circ}$ for $OCl^{-}/ Cl^{-}$ and for $Cl^{-}/ 1/2 Cl_{2}$ are $0.86\ V$ and $-1.10$ volt respectively. The $E^{\circ}$ value of $OCl^{-}/ 1/2Cl_{1}$ will be ?

Question 22 : A galvanic cell is constructed using the redox reaction,&#160;it is represented as:<br/>$\frac{1}{2}H_2(g)+AgCl(s)\rightleftharpoons H^+(aq)+Cl^-(aq)+Ag(s)$<br/>

Question 24 : ${ Cu }^{ + }\left( aq \right) $ is unstable in solution and undergoes simultaneous oxidation and reduction, according to the reaction<br/>$2{ Cu }^{ + }\left( aq \right) \rightleftharpoons { Cu }^{ 2+ }\left( aq \right) +Cu\left( s \right) $<br/>Choose correct ${ E }^{ }$ for above reaction if<br/>${ E }_{ { { Cu }^{ 2+ } }/{ Cu } }^{ }=0.34V$ and ${ E }_{ { { cu }^{ 2+ } }/{ { Cu }^{ + } } }^{ }=0.15V$

Question 25 : $Zn_{(s)} | Zn^{2+}_{(aq)}(1M) || Ni^{2+}_{(aq)}(1M) |Ni_{(s)}$<br/><br/><div>Which is incorrect for the above given cell?</div>

Question 26 : Which of the following statement is not correct about an inert electrode in a cell?

Question 27 : The efficiency of a fuel cell is $80\%$ and the standard heat of reaction is $-300 kJ$. The reaction involves two electrons in redox change. $E^{\ominus}$ for the cell is:

Question 28 : The chemical reaction, $2AgCl_{(s)} + H_{2(g)} \rightarrow 2HCl_{(aq)} + 2Ag_{(s)}$ taking place in a galvanic cell is represented by the notation :

Question 29 : If the solution of $CuSO_4$ in which copper rod is immersed is diluted to $10 $ times , the reduction electode potential:<br/>${ E }_{ Cu^{ +2 }/Cu }^{ \circ&#160; }$ = $0.34 V $<br/>

Question 30 : Assertion: A metal having negative reduction potrential when dipped in the solution of its own ions has a tendency to pass into solution. Reason: Metals undergo reduction.

Question 31 : 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 32 : Which of the following is not true for a galvanic cell when written in an abbreviated form?

Question 33 : Assertion: $E_{Cell}$ should have a positive value for the cell to function. Reason: $E_{cathode} &lt; E_{anode}$.

Question 34 : Assertion: The transfer of electrons from zinc to copper takes place through metal wire connecting the two rods. Reason: Electricity from solution in one beaker to other flows by migration of ions through the salt bridge.

Question 35 : <div>Calculate $E^{\circ}$ values of the following reactions.<br/></div>&#160; &#160;$2Ag + Zn^{2+} \rightarrow &#160;2Ag^+ + Zn$<br/><div>Given that:&#160;$E^{\circ}_{Ag^{+}/Ag}=0.80 V, E^{\circ}_{Zn^{2+}/Zn}=-0.76 V$</div>

Question 36 : The oxidation potential of a hydrogen electrode at $pH = 10$ and $P_{H_2}$ = 1 atm is:

Question 37 : ${E}^{o}$ for the half cell ${ Zn }^{ 2+ }|Zn$, the emf of the cell&#160; $Zn|{ Zn }^{ 2+ }(1M)\parallel 2{ H }^{ + }(1M)|{ H }_{ 2 }(1\ atm)$ is:

Question 38 : At $298\ K$, given that:<div><br/>$Cu(s) |Cu^{2+} (1.0\ M)| |Ag^+ (1.0\ M)| Ag(s)$&#160; &#160; &#160; &#160; &#160; &#160; $E^o_{cell} = 0.46\ V$</div><div><br/>$Zn(s) |Zn^{2+} (1.0\ M)| |Cu^{2+} (1.0\ M)| Cu(s)$&#160; &#160; &#160; &#160; &#160; $E^o_{cell} = 1.10\ V$</div><div><br/>Then, the $E_{cell}$ for the following reaction at&#160;$298 K$ will be:&#160;</div><div><br/>$Zn(s) |Zn^{2+} (0.1\ M)| |Ag^+ (1. 0\ M)| Ag(s)$<br/></div>

Question 40 : The standard reduction potential of metals X, Y and Z are - 0.403 V, 0.337 V and 0.79 V respectively. Which of the following reaction is not possible?

Question 41 : The equilibrium constant for the following reaction at $25^o$C is $2.9\times 10^9$. Calculate standard voltage of the cell.&#160;<div>$Cl_{2(g)}+Br^-_{(aq)}\rightleftharpoons 2Cl^-_{(aq)}$</div>

Question 43 : $E^o$ 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 44 : $E^o$ of an electrode half reaction is related to $\Delta G^o$ by the equation, $E^o=-\Delta G^o/nF$. If the amount of $Ag^+$ in the half reaction $Ag^++e^-\rightarrow Ag$ is tripled then:

Question 45 : <div>State True or False.<br/></div>The absolute value of standard single electrode potential can be determined experimentally.

Question 46 : Given (i)&#160;${ Cu }^{ 2+ }+{ 2e }^{ - }\rightarrow Cu,\quad \quad { E }^{ o }=+0.337V$<div><br/>(ii)&#160;${ Cu }^{ 2+ }+ e^-\rightarrow Cu^+\quad \quad \quad { E }^{ o }=+0.153V$</div><div><br/>Electrode potential, ${ E }^{ 0 }$ for the reaction will be:<br/>${ Cu }^{ + }+{ e }^{ - }\rightarrow Cu$<br/></div>

Question 47 : In the reaction, <br/>$2Al(s) + 6HCl(aq)\rightarrow2Al^{3+}(aq.) + 6Cl^- (aq.) + 3H_2(g)$:<br/>

Question 48 : If $Cu$ reacts with conc. $H_2SO_4$, then what reactions take place:

Question 49 : Four alkali metals A, B, C and D are having respectively standard electrode potentials as -3.05, -1.66, -0.40 and 0.80 V. Which one will be most reducing?

Question 50 : For the electrode process,<br/>$H^{+}+e=\dfrac{1}{2}H_{2}; E_{H_{H}^{+}H_{2}}=x\ volt$<br/>then for $2H^{+}+2e=H_{2}; E_{2H^{+},H_{2}}$ is equal to<br/>