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]
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]
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]
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
doneclear
B)
more voltage is required to reduce \[{{H}^{+}}\] at Hg than at Pt
doneclear
C)
Na is dissolved in Hg while it does not dissolved in Pt
doneclear
D)
concentration of \[{{H}^{+}}\] ions is larger when Pt electrode is taken
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: \[F=96500\,\,C\,mo{{l}^{-1}};\]\[R=8.314\,J{{K}^{-1}}mo{{l}^{-1}})\]
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)
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]
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]
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
doneclear
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.
doneclear
C)
infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte.
doneclear
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.
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]
\[A{{l}_{2}}{{O}_{3}}\] 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 \[Al=27\,g\,mo{{l}^{-1}}\])
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]
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 conductances at infinite dilution of the respective ions? [AIPMT (M) 2010]
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]
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]
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]
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 \[{{I}^{-}}\]
doneclear
B)
There will be no redox reaction
doneclear
C)
\[{{I}^{-}}\] will be oxidised to \[{{I}_{2}}\]
doneclear
D)
\[F{{e}^{2+}}\] will be oxidised to \[F{{e}^{3+}}\]
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]
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]
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]
question_answer37) A device that converts energy of combustion of fuels like hydrogen and methane, directly into electrical energy is known as [NEET 2015 ]
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]
\[Zn|ZnS{{O}_{4}}(0.01)||CuS{{O}_{4}}(1.0\,M)Cu,\] 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 \[{{E}_{2}}\]?
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]
\[2F{{e}^{3+}}(aq)+2{{I}^{}}(aq)\to 2F{{e}^{2+}}(aq)+{{I}_{2}}(aq)\]\[E_{cell}^{\Theta }\text{ }E=0.24\text{ }Vat\text{ }298\text{ }K\]. The standard Gibbs energy \[({{\Delta }_{r}}{{G}^{\Theta }})\] of the cell reaction is:
[Given that Faraday constant\[F=96500\text{ }C\text{ }mo{{l}^{1}}\]]