Solved papers for NEET Chemistry NEET PYQ-Electrochemistry

done NEET PYQ-Electrochemistry Total Questions - 45

• question_answer1) For the cell reaction,             \[C{{u}^{2+}}({{C}_{1}}\,aq)+Zn(s)\rightleftharpoons Z{{n}^{2+}}({{C}_{2}}\,aq)+Cu(s)\] of an electrochemical cell. The change in free energy \[(\Delta G)\] at a given temperature is a function of: [AIPMT 1998]
  A)
  In \[({{C}_{1}})\]
  done clear
  B)
  In \[({{C}_{2}}/{{C}_{1}})\]
  done clear
  C)
  In\[({{C}_{2}})\]
  done clear
  D)
  In \[({{C}_{1}}+{{C}_{2}})\]
  done clear
  View Answer play_arrow

• question_answer2) Without losing its concentration \[ZnC{{l}_{2}}\] solution cannot be kept in contact with:  [AIPMT 1998]
  A)
  Au
  done clear
  B)
  Al
  done clear
  C)
  Pb
  done clear
  D)
  Ag
  done clear
  View Answer play_arrow

• question_answer3) The specific conductance of a 0.1 N KCl solution at \[23{}^\circ C\] is \[0.012\,\,oh{{m}^{-1}}c{{m}^{-1}}\]. The resistance of cell containing the solution at the same temperature was found to be 55 ohm. The cell constant will be: [AIPMT 1999]
  A)
  \[0.142\text{ }c{{m}^{-1}}\]
  done clear
  B)
  \[0.66\text{ }c{{m}^{-1}}\]
  done clear
  C)
  \[0.918\text{ }c{{m}^{-1}}\]
  done clear
  D)
  \[1.12\text{ }c{{m}^{-1}}\]
  done clear
  View Answer play_arrow

• question_answer4) The equivalent conductances of \[B{{a}^{2+}}\] and \[C{{l}^{-}}\]  are 127 and 76 \[oh{{m}^{-1}}\,\,c{{m}^{-1}}\,e{{q}^{-1}}\] respectively at infinite dilution. The equivalent conductance of \[BaC{{l}_{2}}\] at infinite dilution will be: [AIPMT 2000]
  A)
  139.5
  done clear
  B)
  203
  done clear
  C)
  279
  done clear
  D)
  101.5
  done clear
  View Answer play_arrow

• question_answer5) Cell reaction is spontaneous when: [AIPMT 2000]
  A)
  \[E_{red}^{o}\]            is negative
  done clear
  B)
  \[E_{red}^{o}\] is positive
  done clear
  C)
  \[\Delta {{G}^{o}}\] is negative
  done clear
  D)
  \[\Delta {{G}^{o}}\] is positive
  done clear
  View Answer play_arrow

• question_answer6) 

  \[C{{u}^{+}}(aq)\] is unstable in solution and undergoes simultaneous oxidation and reduction according to the reaction:

  \[2C{{u}^{+}}(aq)C{{u}^{2+}}(aq)+Cu(s)\]

  choose correct \[{{E}^{o}}\] for above reaction if \[E_{C{{u}^{2+}}/Cu}^{0}=0.34\,V\] and \[E_{C{{u}^{2+}}/C{{u}^{+}}}^{0}=0.15\,V\] [AIPMT 2000]

  A)
  \[\,0.38\text{ }V\]
  done clear
  B)
  \[+\text{ }0.49\text{ }V\]          
  done clear
  C)
  \[+\text{ }0.38\text{ }V\]
  done clear
  D)
  \[-\text{ }0.19\text{ }V\]
  done clear
  View Answer play_arrow

• question_answer7) 

  Standard electrode potentials are: [AIPMT 2001]

  \[F{{e}^{2+}}/Fe,\]                 \[{{E}^{o}}=-0.44\]

  \[F{{e}^{3+}}/F{{e}^{2+}},\]                       \[{{E}^{o}}=0.77\]

  \[F{{e}^{2+}},\,F{{e}^{3+}}\] and Fe block are kept together, then:

  A)
  \[F{{e}^{3+}}\] increases
  done clear
  B)
  \[F{{e}^{3+}}\] decreases
  done clear
  C)
  \[\frac{F{{e}^{2+}}}{F{{e}^{3+}}}\] remains unchanged       
  done clear
  D)
  \[F{{e}^{2+}}\] decreases
  done clear
  View Answer play_arrow

• question_answer8) The most convenient method to protect the bottom of ship made of iron is:   [AIPMT 2001]
  A)
  coating it with red lead oxide       
  done clear
  B)
  white tin plating
  done clear
  C)
  connecting it with Mg block                     
  done clear
  D)
  connecting it with Pb block
  done clear
  View Answer play_arrow

• question_answer9) In electrolysis of \[NaCl\] when Pt electrode is taken then \[{{H}_{2}}\] is liberated at cathode while with Hg cathode it forms sodium amalgam: [AIPMT 2002]
  A)
  Hg is more inert than Pt  
  done clear
  B)
  more voltage is required to reduce \[{{H}^{+}}\] at Hg than at Pt
  done clear
  C)
  Na is dissolved in Hg while it does not dissolved in Pt
  done clear
  D)
  concentration of \[{{H}^{+}}\] ions is larger when Pt electrode is taken
  done clear
  View Answer play_arrow

• question_answer10) The standard emf of a galvanic cell involving cell reaction with \[n=2\] is found to be 0.295 V at \[25{}^\circ \text{ }C\]. The equilibrium constant of the reaction would be:                         [AIPMT (S) 2004] (Given: \[F=96500\,\,C\,mo{{l}^{-1}};\]\[R=8.314\,J{{K}^{-1}}mo{{l}^{-1}})\]
  A)
  \[2.0\times {{10}^{11}}\]
  done clear
  B)
  \[4.0\times {{10}^{12}}\]
  done clear
  C)
  \[1.0\times {{10}^{2}}\]
  done clear
  D)
  \[1.0\times {{10}^{10}}\]
  done clear
  View Answer play_arrow

• question_answer11) The mass of carbon anode consumed (giving only carbondioxide) in the production of 270 kg of aluminium metal from bauxite by the Hall process is:                                   [AIPMT (S) 2005]             (Atomic mass Al = 27)
  A)
  180 kg
  done clear
  B)
  270 kg
  done clear
  C)
  540 kg
  done clear
  D)
  90 kg
  done clear
  View Answer play_arrow

• question_answer12) 4.5 g of aluminium (at. mass 27 amu) is deposited at cathode from  solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from  ions in solution by the same quantity of electric charge will be:                                [AIPMT (S) 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
  View Answer play_arrow

• question_answer13) If \[E_{F{{e}^{2+}}/Fe}^{o}=-0.441\,V\] and \[E_{F{{e}^{3+}}/F{{e}^{2+}}}^{o}=0.771\,V,\] the standard emf of the reaction:   \[Fe+2F{{e}^{3+}}\to ~3F{{e}^{2+}}\]will be: [AIPMT (S) 2006]
  A)
        0.330 V
  done clear
  B)
  1.653 V
  done clear
  C)
  1.212 V
  done clear
  D)
  0.111 V
  done clear
  View Answer play_arrow

• question_answer14) 

  A hypothetical electrochemical cell is shown below \[A|{{A}^{+}}(xM)||{{B}^{+}}(yM)|B\].

  The emf measured is + 0.20 V. The cell reaction is:                                          [AIPMT (S) 2006]

  A)
  \[{{A}^{+}}+B\xrightarrow{{}}A+{{B}^{+}}\]                                
  done clear
  B)
  \[{{A}^{+}}+{{e}^{-}}\xrightarrow{{}}A;\,{{B}^{+}}+{{e}^{-}}\to B\]
  done clear
  C)
  the cell reaction cannot be predicted         
  done clear
  D)
  \[A+{{B}^{+}}\xrightarrow{{}}{{A}^{+}}+B\]
  done clear
  View Answer play_arrow

• question_answer15) 

  On the basis of the following \[E{}^\circ \] values, the strongest oxidising agent is   [AIPMT (S) 2008]

  \[{{[Fe{{(CN)}_{6}}]}^{4-}}\to {{[Fe{{(CN)}_{6}}]}^{3-}}]+{{e}^{-}};\]\[{{E}^{o}}=-0.35V\]

  \[F{{e}^{2+}}\to F{{e}^{3+}}+{{e}^{-}};{{E}^{o}}=-0.77V\]

  A)
  \[{{[Fe{{(CN)}_{6}}]}^{4-}}\]
  done clear
  B)
  \[F{{e}^{2+}}\]
  done clear
  C)
  \[F{{e}^{3+}}\]
  done clear
  D)
  \[{{[Fe{{(CN)}_{6}}]}^{3-}}\]
  done clear
  View Answer play_arrow

• question_answer16) Kohlrausch's law states that at [AIPMT (S) 2008]
  A)
  finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte
  done clear
  B)
  in finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte depending on the nature of the other ion of the electrolyte.
  done clear
  C)
  infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte.
  done clear
  D)
  infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte.
  done clear
  View Answer play_arrow

• question_answer17) Standard free energies of formation (in kJ/mol) at 298 K are \[-237.2,\text{ }-394.4\] and \[-8.2\] for\[{{H}_{2}}O(l)C{{O}_{2}}(g)\] ate) and pentane (g), respectively. The value of \[E_{cell}^{o}\] pentane-oxygen fuel cell is                           [AIPMT (S) 2008]
  A)
  1.968 V
  done clear
  B)
  2.0968 V
  done clear
  C)
  1.0968 V
  done clear
  D)
  0.0968 V
  done clear
  View Answer play_arrow

• question_answer18) 

  \[A{{l}_{2}}{{O}_{3}}\] is reduced by electrolysis at low potentials and high currents. If \[4.5\times {{10}^{4}}\] A of current is passed through molten \[A{{l}_{2}}{{O}_{3}}\] for 6 h what mass of aluminium is produced?     [AIPMT (S) 2009]

  (Assume 100% current efficiency at. mass of \[Al=27\,g\,mo{{l}^{-1}}\])

  A)
  \[9.0\times {{10}^{3}}\,g\]
  done clear
  B)
  \[8.1\times {{10}^{4}}\,g\]
  done clear
  C)
  \[2.4\times {{10}^{5}}\,g\]
  done clear
  D)
  \[1.3\times {{10}^{4}}\,g\]
  done clear
  View Answer play_arrow

• question_answer19) The equivalent conductance of \[\frac{M}{32}\] solution of a weak monobasic acid is \[8.0\text{ }mho\text{ }c{{m}^{2}}\] and at infinite dilution is \[400\text{ }mho\text{ }c{{m}^{2}}\]. The dissociation constant of this acid is [AIPMT (S) 2009]
  A)
  \[1.25\times {{10}^{-5}}\]
  done clear
  B)
  \[1.25\times {{10}^{-6}}\]
  done clear
  C)
  \[6.25\times {{10}^{-4}}\]
  done clear
  D)
  \[1.25\times {{10}^{-4}}\]
  done clear
  View Answer play_arrow

• question_answer20) 

  Given,                               [AIPMT (S) 2009]

  (i) \[C{{u}^{2+}}+2{{e}^{-}}\xrightarrow[{}]{{}}Cu,\]\[{{E}^{o}}=0.337\,V\]

  (ii) \[C{{u}^{2+}}+{{e}^{-}}\xrightarrow[{}]{{}}C{{u}^{+}},\]\[{{E}^{o}}=0.153\,V\]

  Electrode potential, \[{{E}^{o}}\] for the reaction,  \[Cu+{{e}^{-}}\xrightarrow[{}]{{}}Cu\], will be -

  A)
  0.52 V
  done clear
  B)
  0.90 V
  done clear
  C)
  0.30 V
  done clear
  D)
  0.38 V
  done clear
  View Answer play_arrow

• question_answer21) 

  For the reduction of silver ions with copper metal, the standard cell potential was found to be \[+\text{ }0.46\,V\] at \[25{}^\circ C\]

  The value of standard Gibbs energy, \[\Delta {{G}^{o}}\] will be \[(F\text{ }=\text{ }96500\text{ }C\text{ }mo{{l}^{-1}})\]    [AIPMT (S) 2010]

  A)
  \[-89.0\text{ }kJ\]
  done clear
  B)
  \[-89.0\text{ }J\]
  done clear
  C)
  \[-44.5\text{ }kJ\]
  done clear
  D)
  \[-98.0k\text{ }J\]
  done clear
  View Answer play_arrow

• question_answer22) An increase in equivalent conductance of a strong electrolyte with dilution is mainly due  to [AIPMT (S) 2010]
  A)
  increase in ionic mobility of ions
  done clear
  B)
  100% ionisation of electrolyte at normal dilution
  done clear
  C)
  increase in both, i.e., number of ions and ionic mobility of ions
  done clear
  D)
  increase in number of ions
  done clear
  View Answer play_arrow

• question_answer23) Which of the following expressions correctly represents the equivalent conductance at infinite dilution of \[A{{l}_{2}}{{(S{{O}_{4}})}_{3}}\]. Given that \[\Lambda {{_{Al}^{o}}^{3+}}\] and \[\Lambda _{SO_{4}^{2-}}^{o}\]  are the equivalent conductance’s at infinite dilution of the respective ions?   [AIPMT (M) 2010]
  A)
  \[2{{\Lambda }^{o}}_{A{{l}^{3+}}}+3{{\Lambda }^{o}}_{so\frac{2-}{4}}\]
  done clear
  B)
  \[{{\Lambda }^{o}}_{A{{l}^{3+}}}+{{\Lambda }^{o}}_{so\frac{2-}{4}}\]
  done clear
  C)
  \[({{\Lambda }^{o}}_{A{{l}^{3+}}}+3{{\Lambda }^{o}}_{so\frac{2-}{4}})\times 6\]
  done clear
  D)
  \[\frac{1}{3}{{\Lambda }^{o}}_{A{{l}^{3+}}}+\frac{1}{2}{{\Lambda }^{o}}_{so\frac{2-}{4}}\]
  done clear
  View Answer play_arrow

• question_answer24) 

  Consider the following relations for emf of a electrochemical cell            [AIPMT (M) 2010]

  [A] Emf of cell = (oxidation potential of anode) (reduction potential of cathode)

  [B] Emf of cell = (oxidation potential of anode) + (reduction potential of cathode)

  [C] Emf of cell = (reduction potential of anode) + (reduction potential of cathode)

  [D] Emf of cell = (oxidation potential of anode)-(0xidation potential of cathode)

  Which of the above relations are correct?

  A)
  and
  done clear
  B)
  and      
  done clear
  C)
  and
  done clear
  D)
  None of these
  done clear
  View Answer play_arrow

• question_answer25) Standard electrode potential of three metals X, Y and Z are -1.2 V, + 0.5 V and -3.0 V respectively. The reducing power of these metal will be [AIPMT (S) 2011]
  A)
  \[Y>X>Z\]
  done clear
  B)
  \[Z>X>Y\]
  done clear
  C)
  \[X>Y>Z\]
  done clear
  D)
  \[Y>Z>X\]
  done clear
  View Answer play_arrow

• question_answer26) If the \[{{E}^{o}}_{cell}\] for a given reaction has a negative value then which of the following gives the correct relationships for the values of \[\Delta {{G}^{o}}\] and \[{{K}_{eq}}\]? [AIPMT (S) 2011]
  A)
  \[\Delta {{G}^{o}}<\,0;\,{{K}_{eq}}>1\]
  done clear
  B)
  \[\Delta {{G}^{o}}<\,0;\,{{K}_{eq}}<1\]
  done clear
  C)
  \[\Delta {{G}^{o}}>\,0;\,{{K}_{eq}}<1\]
  done clear
  D)
  \[\Delta {{G}^{o}}>\,0;\,{{K}_{eq}}>1\]
  done clear
  View Answer play_arrow

• question_answer27) 

  The electrode potentials for [AIPMT (S) 2011]

  \[C{{u}^{2+}}(aq)+{{e}^{-}}\xrightarrow[{}]{{}}C{{u}^{+}}(aq)\] and\[C{{u}^{+}}(aq)+{{e}^{-}}\xrightarrow[{}]{{}}Cu(s)\]

  Are + 0.15 V and + 0.50 v respectively. The value of \[{{E}^{o}}_{C{{u}^{2+}}/Cu}\] will be

  A)
  0.325 V
  done clear
  B)
  0.650 V
  done clear
  C)
  0.150 V
  done clear
  D)
  0.500 V
  done clear
  View Answer play_arrow

• question_answer28) Standard electrode potential for \[S{{n}^{4+}}/S{{n}^{2+}}\] couple is +0.15 V and that for the \[C{{r}^{3+}}/Cr\] couple is -0.74. These two couples in their standard state are connected to make a cell. The cell potential will be              [AIPMT (S) 2011]
  A)
  + 0.89 V
  done clear
  B)
  + 0.18 V
  done clear
  C)
  + 1.83 V
  done clear
  D)
  + 1.199 V
  done clear
  View Answer play_arrow

• question_answer29) A solution contains \[F{{e}^{2+}},F{{e}^{3+}}\] and \[{{I}^{-}}\] ions. This solution was treated with iodine at \[35{}^\circ C\]. \[E{}^\circ \] for \[F{{e}^{3+}}/F{{e}^{2+}}\] is + 0.77 V and \[E{}^\circ \] for \[{{I}_{2}}/2{{I}^{-}}=0.536\,V\]. The favorable redox reaction is                       [AIPMT (M) 2011]
  A)
  \[{{I}_{2}}\] will be reduced to \[{{I}^{-}}\]
  done clear
  B)
  There will be no redox reaction
  done clear
  C)
  \[{{I}^{-}}\] will be oxidised to \[{{I}_{2}}\]
  done clear
  D)
  \[F{{e}^{2+}}\] will be oxidised to \[F{{e}^{3+}}\]
  done clear
  View Answer play_arrow

• question_answer30) Limiting molar conductivity of \[N{{H}_{4}}OH\] \[(i.e.,\,\Delta {{m}_{(N{{H}_{4}}Cl)}})\] is equal to    [AIPMT (S) 2012]
  A)
  \[{{\Lambda }_{m(N{{H}_{4}}Cl)}}+{{\overset{o}{\mathop{\Lambda }}\,}_{m(NaCl)}}-{{\overset{o}{\mathop{\Lambda }}\,}_{m(NaOH)}}\]
  done clear
  B)
  \[{{\overset{o}{\mathop{\Lambda }}\,}_{m}}_{(NaOH)}+{{\overset{o}{\mathop{\Lambda }}\,}_{m(NaCl)}}-{{\overset{o}{\mathop{\Lambda }}\,}_{m(N{{H}_{4}}Cl)}}\]
  done clear
  C)
  \[{{\overset{o}{\mathop{\Lambda }}\,}_{m(N{{H}_{4}}OH)}}+{{\overset{o}{\mathop{\Lambda }}\,}_{m(N{{H}_{4}}Cl)}}-{{\overset{o}{\mathop{\Lambda }}\,}_{m(HCl)}}\]
  done clear
  D)
  \[{{\overset{o}{\mathop{\Lambda }}\,}_{m(N{{H}_{4}}OH)}}+{{\overset{o}{\mathop{\Lambda }}\,}_{m(NaOH)}}-{{\overset{o}{\mathop{\Lambda }}\,}_{m(NaCl)}}\]
  done clear
  View Answer play_arrow

• question_answer31) 

  Standard reduction potentials of the half reactions are given below                    [AIPMT (M) 2012]

  \[{{F}_{2}}(g)=2{{e}^{-}}\xrightarrow[{}]{{}}2{{F}^{-}}(aq);\]\[{{E}^{o}}=+\,2.85\,V\]\[C{{l}_{2}}(g)+2{{e}^{-}}\xrightarrow[{}]{{}}2C{{l}^{-}}(aq);\]\[{{E}^{o}}=+\,1.36\,V\]

  \[B{{r}_{2}}(l)+2{{e}^{-}}\xrightarrow[{}]{{}}2B{{r}^{-}}(aq);\]\[{{E}^{o}}=+1.06\,V\]

  \[{{I}_{2}}(s)+2{{e}^{-}}\xrightarrow[{}]{{}}2{{I}^{-}}(aq);\]\[{{E}^{o}}=+0.53\,V\]

  The strongest oxidsing and reducing agents respectively are

  A)
                               \[{{F}_{2}}\] and \[{{I}^{-}}\]
  done clear
  B)
  \[B{{r}_{2}}\] and \[C{{l}^{-}}\]
  done clear
  C)
  \[C{{l}_{2}}\] and \[B{{r}^{-}}\]
  done clear
  D)
  \[C{{l}_{2}}\] and \[{{I}_{2}}\]
  done clear
  View Answer play_arrow

• question_answer32) Molar conductivities  at infinite dilution of  and   are 126.4, 425.9 and  respectively.  for  will be      [AIPMT (M) 2012]
  A)
  
  done clear
  B)
  \[180.5\,\,S\,\,c{{m}^{2}}\,mo{{l}^{-1}}\]
  done clear
  C)
  \[290.8\,\,S\,\,c{{m}^{2}}\,mo{{l}^{-1}}\]
  done clear
  D)
  \[390.5\,\,S\,\,c{{m}^{2}}\,mo{{l}^{-1}}\]
  done clear
  View Answer play_arrow

• question_answer33) A hydrogen gas electrode is made by dipping platinum wire in a solution of \[HCl\] of \[pH=10\] and by passing hydrogen gas around the platinum wire at 1 atm pressure. The oxidation potential of electrode would be        [NEET 2013]
  A)
  0.059 V
  done clear
  B)
  0.59 V
  done clear
  C)
  0.118 V
  done clear
  D)
  1.18 V
  done clear
  View Answer play_arrow

• question_answer34) At \[25{}^\circ C\] molar conductance of 0.1 molar aqueous   solution   of ammonium hydroxide is \[9.54\,\,\,oh{{m}^{-1}}\,\,c{{m}^{2}}\,\,mo{{l}^{-1}}\] and at infinite dilution its molar conductance is \[238\,\,oh{{m}^{-1}}\,c{{m}^{2}}\,mo{{l}^{-1}}\]. The degree of ionization of ammonium hydroxide at the same concentration and temperature is [NEET 2013]  
  A)
  2.080%
  done clear
  B)
  20.800%
  done clear
  C)
  4.008%
  done clear
  D)
  40.800%
  done clear
  View Answer play_arrow

• question_answer35) 

  A button cell used in watches functions as following                                     [NEET 2013]

  \[Zn(s)+A{{g}_{2}}O(s)+{{H}_{2}}O(l)2Ag(s)\]\[+Z{{n}^{2+}}(aq)+2O{{H}^{-}}(aq)\]

  If half cell potentials are

  \[Z{{n}^{2+}}(aq)+2{{e}^{-}}\to Zn(s){{E}^{o}}=-0.76V\]\[A{{g}_{2}}O(s)+{{H}_{2}}O(l)+2{{e}^{-}}\]\[\to 2Ag(s)+2O{{H}^{-}}(aq),\]\[{{E}^{o}}=0.34V\]

  The cell potential will be

  A)
  1.10 V
  done clear
  B)
  0, 42 V
  done clear
  C)
  0.84 V
  done clear
  D)
  1.34 V
  done clear
  View Answer play_arrow

• question_answer36) The weight of silver (at. wt. = 108) displaced by a quantity of electricity which displaces 5600 mL of \[{{O}_{2}}\] at STP will be                    [AIPMT 2014]
  A)
  5.4 g
  done clear
  B)
  10.8 g
  done clear
  C)
  54.0 g
  done clear
  D)
  108.0 g
  done clear
  View Answer play_arrow

• question_answer37) A device that converts energy of combustion of fuels like hydrogen and methane, directly into electrical energy is known as [NEET 2015 ]
  A)
  fuel cell
  done clear
  B)
  electrolytic cell
  done clear
  C)
  dynamo
  done clear
  D)
  Ni-Cd cell
  done clear
  View Answer play_arrow

• question_answer38) 2, 3-dimethyl-2-butene can be prepared by heating which of the following compounds with a strong acid?                             [NEET 2015 (Re)]
  A)
  \[{{(C{{H}_{3}})}_{2}}CH-\underset{\underset{C{{H}_{3}}}{\mathop{|}}\,}{\mathop{CH}}\,-CH=C{{H}_{2}}\]
  done clear
  B)
  \[{{(C{{H}_{3}})}_{3}}C-CH=C{{H}_{2}}\]
  done clear
  C)
  \[{{(C{{H}_{3}})}_{2}}C=CH-C{{H}_{2}}-C{{H}_{3}}\]
  done clear
  D)
  \[{{(C{{H}_{3}})}_{2}}CH-C{{H}_{2}}-CH=C{{H}_{2}}\]
  done clear
  View Answer play_arrow

• question_answer39) The pressure of \[{{H}_{2}}\] required to make the potential of \[{{H}_{2}}-\] electrode zero in pure water at 298 K is :-[NEET - 2016]
  A)
  \[{{10}^{14}}\text{ }atm\]
  done clear
  B)
  \[{{10}^{12}}\text{ }atm\]
  done clear
  C)
  \[{{10}^{-10}}atm\]
  done clear
  D)
  \[{{10}^{-4}}atm\]
  done clear
  View Answer play_arrow

• question_answer40) 

  In the electrochemical cell [NEET-2017]

  \[Zn|ZnS{{O}_{4}}(0.01)||CuS{{O}_{4}}(1.0\,M)Cu,\] the emf of this Daniel cell is \[{{E}_{1}}\]. When the concentration of \[ZnS{{O}_{4}}\] is changed to 1.0 M and that of \[CuS{{O}_{4}}\] changed to 0.01 M, emf changes to \[{{E}_{2}}\]. From the following, which one is the relationship between\[{{E}_{1}}\] and \[{{E}_{2}}\]?

  (Given, \[\frac{RT}{F}=0.059\])

  A)
  \[{{E}_{2}}=0\ne {{E}_{1}}\]
  done clear
  B)
  \[{{E}_{1}}={{E}_{2}}\]
  done clear
  C)
  \[{{E}_{1}}<{{E}_{2}}\]
  done clear
  D)
  \[{{E}_{1}}>{{E}_{2}}\]
  done clear
  View Answer play_arrow

• question_answer41) 

  Consider the change in oxidation state of Bromine corresponding to different emf values as shown in the diagram below: [NEET - 2018]

  Then the species undergoing disproportionation is

  A)
  \[\text{B}{{\text{r}}_{2}}\]  
  done clear
  B)
  \[\text{BrO}_{\text{4}}^{\text{-}}\]
  done clear
  C)
  \[\text{BrO}_{\text{3}}^{\text{-}}\]
  done clear
  D)
  \[\text{HBrO}\]
  done clear
  View Answer play_arrow

• question_answer42) 

  For a cell involving one electron  \[E_{cell}^{\Theta }=0.59\text{ }V\text{ }at\text{ }298\text{ }K\], the equilibrium constant for the cell reaction is:

  [Given that \[\frac{2.303kT}{F}=0.059\text{ }V\text{ }at\text{ }T=298\text{ }K\]] [NEET 2019]

  A)
  \[1.0\times {{10}^{10}}\]
  done clear
  B)
  \[1.0\times {{10}^{30}}\]
  done clear
  C)
  \[1.0\times {{10}^{2}}\]
  done clear
  D)
  \[1.0\times {{10}^{5}}\]
  done clear
  View Answer play_arrow

• question_answer43) 

  For the cell reaction                      [NEET 2019]

  \[2F{{e}^{3+}}(aq)+2{{I}^{}}(aq)\to 2F{{e}^{2+}}(aq)+{{I}_{2}}(aq)\]\[E_{cell}^{\Theta }\text{ }E=0.24\text{ }Vat\text{ }298\text{ }K\]. The standard Gibbs energy \[({{\Delta }_{r}}{{G}^{\Theta }})\] of the cell reaction is:

  [Given that Faraday constant\[F=96500\text{ }C\text{ }mo{{l}^{1}}\]]

  A)
  \[46.32\text{ }kJ\text{ }mo{{l}^{1}}\]
  done clear
  B)
  \[23.16\text{ }kJ\text{ }mo{{l}^{1}}\]
  done clear
  C)
  \[-46.32\text{ }kJ\text{ }mo{{l}^{1}}\]
  done clear
  D)
  \[-23.16\text{ }kJ\text{ }mo{{l}^{1}}\]
  done clear
  View Answer play_arrow

• question_answer44) 

  The number of Faradays(F) required to produce 20 g of calcium from molten \[CaC{{l}_{2}}\]

  (Atomic mass of\[Ca=40\text{ }g\text{ }mo{{l}^{1}}\]) is [NEET 2020]

  A)
  2
  done clear
  B)
  3
  done clear
  C)
  4
  done clear
  D)
  1
  done clear
  View Answer play_arrow

• question_answer45) On electrolysis of dil. sulphuric acid using Platinum (Pt) electrode, the product obtained at anode will be[NEET 2020]
  A)
  Oxygen gas
  done clear
  B)
  \[{{H}_{2}}S\] gas
  done clear
  C)
  \[S{{O}_{2}}\] gas
  done clear
  D)
  Hydrogen gas
  done clear
  View Answer play_arrow