Question 1 :
In acidic medium $ Cr_{2}O_{7}^{-2} $ is an oxiding agent <br/>$Cr_{2}O_{7}^{-2}+14 H^{+}+6e^{-}\leftarrow 2Cr^{+3}+7H_{2}O$<br/>$[E^{^{\circ}}_{Cr_{2}O_{7}^{-2}/Cr^{+3}}=1.33 V]$<br/>The electrode potential of half cell at $pH=1$ keeping concentration of other species unity is:
Question 2 : At $298\ K$, given that:<div><br/>$Cu(s) |Cu^{2+} (1.0\ M)| |Ag^+ (1.0\ M)| Ag(s)$            $E^o_{cell} = 0.46\ V$</div><div><br/>$Zn(s) |Zn^{2+} (1.0\ M)| |Cu^{2+} (1.0\ M)| Cu(s)$          $E^o_{cell} = 1.10\ V$</div><div><br/>Then, the $E_{cell}$ for the following reaction at $298 K$ will be: </div><div><br/>$Zn(s) |Zn^{2+} (0.1\ M)| |Ag^+ (1. 0\ M)| Ag(s)$<br/></div>
Question 3 :
Assertion: The standard reduction potential for $Ag^+ + e^- \rightarrow Ag$ is half that of $2Ag^+ + 2e^- \rightarrow 2Ag$
Reason: Standard potential is dependent on the number of electrons transferred
Question 4 :
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} $. The reduction potential of aluminium electrode is
Question 5 :
The oxidation potential of hydrogen electrode at pH = 10 and P$_{H_2}$ = 1 atm is __________.
Question 8 :
Given<br/>$E^{\circ}_{Cr^{3+}/ Cr} = -0.74\ V; E^{\circ}_{MnO_{4}^{-}/ Mn^{2+}} = + 1.51\ V$<br/>$E^{\circ}_{Cr_{2}O_{7}^{2-}/ Cr^{3+}} = + 1.33\ V; E^{\circ}_{Cl/ Cl^{-}} = + 1.36\ V$<br/>based on the data given above, strongest oxidizing agent will be__________.
Question 9 : <b>Question below</b> refers to the overall reaction and half-reactions with standard reduction potentials below.<br/>$2Fe^{2+} + Cl_2 \rightarrow 2Fe^{3+} + 2Cl$?<br/>$Fe^{3+} + e^- \rightarrow Fe^{2+}$; $E^o_{red}$ = 0.77 volts<br/>$Cl_2 + 2e^- \rightarrow 2Cl^-$ ; $E^o_{red}$ = 1.36 volts<br/><div>Find the overall potential for the reaction ?</div>
Question 10 : 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 11 :
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 12 :
If the $H^+$ concentration decreased from 1 M to $10^{-4}$ M at $25^oC$ for the couple $MnO_4^-/ Mn^{2+}$, then the oxidising power of the $MnO_4^-/ Mn^{2+}$ couple decreases by
Question 13 :
The standard reduction potential of the reaction, $H_2O+e^-\rightarrow \displaystyle\frac{1}{2}H_2+OH$ at $298$K is:
Question 15 :
$E^o$ 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 17 :
In the reaction, <br/>$2Al(s) + 6HCl(aq)\rightarrow2Al^{3+}(aq.) + 6Cl^- (aq.) + 3H_2(g)$:<br/>
Question 18 :
The oxidation potential of $Zn, Cu, Ag, { H }_{ 2 }$ and $Ni$ are 0.76, -0.34, -0.80, 0, 0.55 volt respectively. Which of the following reaction will provide maximum voltage?
Question 19 :
Which one is correct about a hypothetical electrochemical cell shown below?<br/>$\underset{A}{\ominus } | A^+ (XM) || B^+ (YM) | \underset{B}{\oplus}           E_{cell}  = + 0.20 V$<br/>
Question 21 :
Which of the following is not true for a galvanic cell when written in an abbreviated form?
Question 22 :
Assertion: A standard hydrogen electrode is also called reversible electrode.
Reason: Standard hydrogen electrode can act both as anode as well as cathode in an electrochemical cell.
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 : <div>Assertion: The absolute value of standard electrode potential can be determined experimentally.</div><div>Reason: Standard electrode potentials are measured using a hydrogen half-cell reference electrode whose potential is known.<br/></div>
