JEE Main & Advanced Chemistry Electrochemistry / विद्युत् रसायन Question Bank

done Critical Thinking Electrochemistry Total Questions - 14

• question_answer1)
  The limiting molar conductivities \[{{\wedge }^{0}}\]for NaCl, KBr and KCl are 126, 152 and 150 \[S\ c{{m}^{2}}mo{{l}^{-1}}\] respectively. The \[{{\wedge }^{0}}\] for NaBr is                                    [AIEEE 2004]
  A)
                  \[278\ S\ c{{m}^{2}}mo{{l}^{-1}}\]            done clear
  B)
                  \[176\ S\ c{{m}^{2}}mo{{l}^{-1}}\] done clear
  C)
                  \[128\ S\ c{{m}^{2}}mo{{l}^{-1}}\]            done clear
  D)
                  \[302\ S\ c{{m}^{2}}mo{{l}^{-1}}\] done clear
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• question_answer2)
  On the basis of the electrochemical theory of aqueous corrosion, the reaction occurring at the cathode is [MP PET 1994; UPSEAT 2001]
  A)
                  \[{{O}_{2\,(g)}}+4H_{(aq)}^{+}+4{{e}^{-}}\to 2{{H}_{2}}{{O}_{(l)}}\] done clear
  B)
                  \[F{{e}_{(s)}}\to Fe_{(aq)}^{2+}+2{{e}^{-}}\] done clear
  C)
                  \[Fe_{(aq)}^{2+}\to Fe_{(aq)}^{3+}+{{e}^{-}}\] done clear
  D)
                  \[{{H}_{2(g)}}+2OH_{(aq)}^{-}\to 2{{H}_{2}}{{O}_{(l)}}+2{{e}^{-}}\] done clear
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• question_answer3)
  The reaction \[\tfrac{1}{2}{{H}_{2}}(g)+AgCl(s)\,\to \,{{H}^{+}}(aq)+C{{l}^{-}}(aq)+Ag(s)\]                 occurs in the galvanic cell                                                 [IIT 1985; AMU 2002; KCET 2003]
  A)
                  \[Ag/AgCl(s)\,KCl\,(\text{soln})\,\,||\,\,AgN{{O}_{3}}\,(\text{soln})\,/Ag\] done clear
  B)
                  \[Pt/{{H}_{2}}(g)\,HCl\,(\text{soln})\,\,||\,\,AgN{{O}_{3}}\,(\text{soln})\,/Ag\] done clear
  C)
                  \[Pt/{{H}_{2}}(g)\,HCl\,(\text{soln})\,\,||\,\,AgCl\,(s)\,/Ag\] done clear
  D)
                  \[Pt/{{H}_{2}}(g)\,KCl\,(\text{soln})\,\,||\,\,AgCl\,(s)\,/Ag\] done clear
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• question_answer4)
  The standard reduction potential \[NaCl\]for the half reactions are as                 \[Zn=Z{{n}^{2+}}+2{{e}^{-}};\,\,{{E}^{o}}=+0.76\,V\]                 \[Fe=F{{e}^{2+}}+2{{e}^{-}};\,\,{{E}^{o}}=+0.41\,V\]                 The EMF for cell reaction \[F{{e}^{2+}}+Zn\,\to \,Z{{n}^{2+}}+Fe\] is [IIT 1988; CBSE PMT 1993, 96; BHU 1995, 2000; CPMT 2000; KCET 2000; AIIMS 2001; Orissa JEE 2002]
  A)
                  \[-\,0.35\,V\]     done clear
  B)
                  \[+\,0.35\,V\] done clear
  C)
                  \[+\,1.17\,V\]    done clear
  D)
                  \[-\,1.17\,V\] done clear
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• question_answer5)
  The number of electrons to balance the following equation \[NO_{3}^{-}+4{{H}^{+}}+{{e}^{-}}\,\to \,2{{H}_{2}}O+NO\] is    [IIT Screening 1991]
  A)
                  5              done clear
  B)
                  4 done clear
  C)
                  3              done clear
  D)
                  2 done clear
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• question_answer6)
  The standard \[EMF\] for the given cell reaction \[Zn+C{{u}^{2+}}=Cu+Z{{n}^{2+}}\] is \[1.10V\] at \[{{25}^{o}}C\]. The \[EMF\] for the cell reaction, when \[0.1M\,C{{u}^{2+}}\] and \[0.1M\,Z{{n}^{2+}}\] solutions are used, at \[{{25}^{o}}C\] is [MNR 1994; AMU 1999; UPSEAT 2002]
  A)
                  \[1.10\,V\]          done clear
  B)
                  \[0.110\,V\] done clear
  C)
                  \[-1.10\,V\]        done clear
  D)
                  \[-\,0.110\,V\] done clear
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• question_answer7)
  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 \[Z>Y>X\], then         [IIT 1999]
  A)
                  \[Y\] will oxidize \[X\] and not \[Z\]                 done clear
  B)
                  \[Y\] will oxidize \[Z\] and not \[X\] done clear
  C)
                  \[Y\] will oxidize both \[X\] and \[Z\] done clear
  D)
                  \[Y\] will reduce both \[X\] and \[Z\] done clear
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• question_answer8)
  The oxidation potential of a hydrogen electrode at pH = 10 and \[p{{H}_{1}}=1\]                                               [JIPMER 2000]
  A)
                  0.059 V done clear
  B)
                  0.59 V done clear
  C)
                  0.00 V    done clear
  D)
                  0.51 V done clear
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• question_answer9)
  The decomposition of hydrogen peroxide is an example of [Roorkee 2000]
  A)
                  Exothermic reaction       done clear
  B)
                  Endothermic reaction done clear
  C)
                  Negative catalysis            done clear
  D)
                  Auto-oxidation done clear
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• question_answer10)
  Aluminium oxide may be electrolysed at 1000°C to furnish aluminium metal (At. Mass = 27 amu; 1 Faraday = 96,500 Coulombs). The cathode reaction is \[A{{l}^{3}}+3{{e}^{-}}\to Al{}^\circ \] To prepare 5.12kg of aluminium metal by this method would require      [AIEEE 2005]
  A)
                  \[5.49\times {{10}^{7}}C\] of electricity  done clear
  B)
   \[1.83\times {{10}^{7}}C\] of electricity done clear
  C)
                  \[5.49\times {{10}^{4}}C\] of electricity done clear
  D)
                  \[5.49\times {{10}^{1}}C\] of electricity done clear
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• question_answer11)
  Calculate \[\Lambda _{HOAc}^{\infty }\] using appropriate molar conductances of the electrolytes listed above at infinite dilution in \[{{H}_{2}}O\] at 25°C                [AIEEE 2005]
  A)
                  517.2     done clear
  B)
                  552.7 done clear
  C)
                  390.7     done clear
  D)
                  217.5 done clear
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• question_answer12)
  The mass of carbon anode consumed (giving only carbondioxide) in the production of 270kg of aluminium metal from bauxite by the Hall process is      [CBSE PMT 2005]
  A)
                  180kg    done clear
  B)
                  270kg done clear
  C)
                  540kg    done clear
  D)
                  90kg done clear
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• question_answer13)
  4.5g of aluminium (at mass 27amu) is deposited at cathode from \[A{{l}^{3+}}\] solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from \[{{H}^{+}}\] ions in solution by the same quantity of electric charge will be [CBSE PMT 2005]
  A)
                  22.4 L     done clear
  B)
                  44.8 L done clear
  C)
                  5.6 L       done clear
  D)
                  11.2 L done clear
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• question_answer14)
  What amount of Cl2 gas liberated at anode, if 1 amp. current is passed for 30 min. from NaCl solution. [BHU 2005]
  A)
                  0.66 moles          done clear
  B)
                  0.33 moles done clear
  C)
                  0.66 g    done clear
  D)
                  0.33 g done clear
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