{"id":19112,"date":"2021-02-20T18:10:11","date_gmt":"2021-02-20T12:40:11","guid":{"rendered":"https:\/\/ncertsolutions.guru\/?p=19112"},"modified":"2021-02-20T18:10:11","modified_gmt":"2021-02-20T12:40:11","slug":"mcq-questions-for-class-12-chemistry-chapter-3","status":"publish","type":"post","link":"https:\/\/ncertsolutions.guru\/mcq-questions-for-class-12-chemistry-chapter-3\/","title":{"rendered":"MCQ Questions for Class 12 Chemistry Chapter 3 Electrochemistry with Answers"},"content":{"rendered":"

Students are advised to practice the NCERT MCQ Questions for Class 12 Chemistry Chapter 3 Electrochemistry with Answers Pdf free download is available here. MCQ Questions for Class 12 Chemistry with Answers<\/a> are prepared as per the Latest Exam Pattern. Students can solve these Electrochemistry Class 12 MCQs Questions with Answers and assess their preparation level.<\/p>\n

Electrochemistry Class 12 MCQs Questions with Answers<\/h2>\n

Solving the Electrochemistry Multiple Choice Questions of Class 12 Chemistry Chapter 3 MCQ can be of extreme help as you will be aware of all the concepts. These MCQ Questions on Electrochemistry Class 12 with answers pave for a quick revision of the Chapter thereby helping you to enhance subject knowledge. Have a glance at the MCQ of Chapter 3 Chemistry Class 12 and cross-check your answers during preparation.<\/p>\n

Question 1.
\nIf the conductivity and conductance of a solution is same then its cell constant is equal to:
\n(a) 1
\n(b) 0
\n(c) 10
\n(d) 1000<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 1<\/p>\n<\/details>\n

\n

Question 2.
\nThe units of conductivity are:
\n(a) ohm-1<\/sup>
\n(b) ohm-1<\/sup> cm-1<\/sup>
\n(c) ohm-2<\/sup> cm\u00b2 equiv-1<\/sup>
\n(d) ohm-1<\/sup> cm\u00b2<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) ohm-1<\/sup> cm-1<\/sup><\/p>\n<\/details>\n

\n

Question 3.
\nThe resistance of 0.1 N solution of acetic acid is 250 ohm, when measured in a cell of cell constant 1.15 cm-1<\/sup>. The equivalent conductance (in ohm-1<\/sup> cm\u00b2 equivalent-1<\/sup>) of 0.1 N acetic acid is
\n(a) 18.4
\n(b) 0.023
\n(c) 46
\n(d) 9.2<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) 46<\/p>\n<\/details>\n

\n

Question 4.
\nIn infinite dilution of aqueous solution of BaCl2<\/sub>, molar conductivity of Ba2+<\/sup> and Cl–<\/sup> ions are = 127.32 S cm\u00b2\/mol and 76.34 S cm2\/mol respectively. What is A\u00b0m for BaCI2 at same dilution?
\n(a) 280 S cm\u00b2 mol-1<\/sup>
\n(b) 330.98 S cm\u00b2 mol-1<\/sup>
\n(c) 90.98 S cm\u00b2 mol-1<\/sup>
\n(d) 203.6 S cm\u00b2 mol-1<\/sup><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 280 S cm\u00b2 mol-1<\/sup><\/p>\n<\/details>\n

\n

Question 5.
\nThe specific conductance of 0.1 M NaCl solution is 1.06 \u00d7 10-2<\/sup> ohm-1<\/sup> cm-1<\/sup>. Its molar conductance in ohm-1<\/sup> cm\u00b2 mol-1<\/sup> is
\n(a) 1.06 \u00d7 10\u00b2
\n(b)1.06 \u00d7 10\u00b3
\n(c) 1.06 \u00d7 104<\/sup>
\n(d) 53<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 1.06 \u00d7 10\u00b2<\/p>\n<\/details>\n

\n

Question 6.
\nThe limiting molar conductivities A\u00b0 for NaCl, KBr and KCl are 126, 152 and 150 S cm\u00b2 mol-1<\/sup> respectively. The A\u00b0 for NaBr is
\n(a) 278 S cm\u00b2 mol-1<\/sup>
\n(b) 976 S cm\u00b2 mol-1<\/sup>
\n(c) 128 S cm\u00b2 mol-1<\/sup>
\n(d) 302 S cm\u00b2 mol-1<\/sup><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) 128 S cm\u00b2 mol-1<\/sup><\/p>\n<\/details>\n

\n

Question 7.
\n\u03bb(CICH2<\/sub>COONa) = 224 ohm-1<\/sup> cm\u00b2 gm eq-1<\/sup>, \u03bb(NaCl) = 38.2 ohm-1<\/sup> cm\u00b2 gm eq-1<\/sup>. \u03bb(HCl) = 203 ohm-1<\/sup> cm\u00b2 gm eq-1<\/sup>, what is the value of \u03bb(CICH2<\/sub>COOH)?
\n(a) 288.5 ohm-1<\/sup> cm\u00b2 gm eq-1<\/sup>
\n(b) 289.5 ohm-1<\/sup> cm\u00b2 gm eq-1<\/sup>
\n(c) 388.8 ohm-1<\/sup> cm\u00b2 gm eq-1<\/sup>
\n(d) 59.5 ohm-1<\/sup> cm\u00b2 gm eq-1<\/sup><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) 388.8 ohm-1<\/sup> cm\u00b2 gm eq-1<\/sup><\/p>\n<\/details>\n

\n

Question 8.
\nThe limiting molar conductivities of HCl, CH3<\/sub>COONa and NaCl are respectively 425, 90 and 125 mho cm\u00b2 mol-1<\/sup> at 25 \u00b0C. The molar conductivity of 0.1 M CH3<\/sub>COOH solution is 7.8 mho cm\u00b2 mol-1<\/sup> at the same temperature. The degree of dissociation of 0.1 M acetic acid solution at the same temperature is
\n(a) 0.10
\n(b) 0.02
\n(c) 0.15
\n(d) 0.03<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) 0.02<\/p>\n<\/details>\n

\n

Question 9.
\nThe values of limiting ionic conductance of H and HCOO–<\/sup> ions are respectively 347 and 53 S cm\u00b2 mol-1<\/sup> at 298 K. If the molar conductance of 0.025 M methanoic acid at 298 K is 40 S cm\u00b2 mol-1<\/sup>, the dissociation constant of methanoic acid at 298 K is
\n(a) 1 \u00d7 10-5<\/sup>
\n(b) 2 \u00d7 10-5<\/sup>
\n(c) 1.5 \u00d7 10-4<\/sup>
\n(d) 2.5 \u00d7 10-4<\/sup><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) 2.5 \u00d7 10-4<\/sup><\/p>\n<\/details>\n

\n

Question 10.
\nThe ionisation constant of a weak electrolyte is 2.5 \u00d7 10-5<\/sup> and molar conductance of its 0.01 M solution is 19.6 S cm\u00b2 mol-1<\/sup>. The molar conductance at infinite dilution (S cm\u00b2 mol-1<\/sup>) is
\n(a) 402
\n(b) 392
\n(c) 306
\n(d) 39.2<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) 392<\/p>\n<\/details>\n

\n

Question 11.
\nWhich of the following statements is incorrect about electrochemical cell?
\n(a) Electrons are released at anode.
\n(b) Chemical energy is converted into electrical energy.
\n(c) Salt bridge maintains the electrical neutrality of the electrolytes.
\n(d) Cell can work indefinitely.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) Cell can work indefinitely.<\/p>\n<\/details>\n

\n

Question 12.
\nPoint out the correct statement in a cell of zinc and copper:
\n(a) Zinc acts as cathode and copper as anode.
\n(b) Zinc acts as anode and copper as cathode.
\n(c) The standard reduction potential of zinc is more than that of copper.
\n(d) The flow of electrons is from copper to zinc.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Zinc acts as anode and copper as cathode.<\/p>\n<\/details>\n

\n

Question 13.
\nThe standard electrode potentials for Pb2+<\/sup>\/Pb and Zn2+\/Zn are – 0.126 V and – 0.763 V respectively. The e.m.f. of the cell Zn | Zn2+<\/sup> (0.1 M) | | Pb2+<\/sup> (0.1 M) | Pb is:
\n(a) 0.637 V
\n(b) < 0.637 V
\n(c) > 0.637 V
\n(d) 0.889 V.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 0.637 V<\/p>\n<\/details>\n

\n

Question 14.
\nA zinc electrode is placed in 0.1 M solution of ZnSO4<\/sub> at 25\u00b0C. Assuming that the salt is dissociated to an extent of 20% at this dilution, the potential of this electrode is (E\u00b0 = -0.76V)
\n(a) – 0.81 V
\n(b) – 0.79 V
\n(c) 0.81 V
\n(d) 0.79 V<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) – 0.81 V<\/p>\n<\/details>\n

\n

Question 15.
\nFor the electrode reaction Mn+<\/sup>(aq) + ne–<\/sup> \u2192 M(s) Nernst equation is
\n(a) E = E\u00b0 + \\(\\frac { RT }{nF}\\) ln \\(\\frac { [m] }{[m^{n+}]}\\)
\n(b) E\u00b0 = E\u00b0 + RT ln [Mn+<\/sup>]
\n(c) E = E\u00b0 + \\(\\frac { RT }{nF}\\) ln [Mn+<\/sup>]
\n(d) \\(\\frac { E }{E\u00b0}\\) = \\(\\frac { RT }{nF}\\) ln [Mn+<\/sup>]<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) E = E\u00b0 + \\(\\frac { RT }{nF}\\) ln [Mn+<\/sup>]<\/p>\n<\/details>\n

\n

Question 16.
\nE\u00b0cell<\/sub> apd \u0394G\u00b0 are related as:
\n(a) \u0394G\u00b0 = nF E\u00b0cell<\/sub>
\n(b) \u0394G = -nF E\u00b0cell<\/sub>
\n(c) \u0394G\u00b0 = -nF E\u00b0cell<\/sub>
\n(d) \u0394G\u00b0 = nF E\u00b0cell<\/sub> = 0.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) \u0394G\u00b0 = -nF E\u00b0cell<\/sub><\/p>\n<\/details>\n

\n

Question 17.
\nWhich of the following will decrease the voltage of the cell?
\nSn(s) + 2Ag+<\/sup> (aq) \u2192 Sn2+<\/sup> (aq) + 2 Ag(s)
\n(a) increase in the size of silver rod
\n(b) increase in the concentration of Sn2+<\/sup> ions
\n(c) increase in the concentration of Ag+<\/sup> ions
\n(d) None of the above.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) increase in the concentration of Sn2+<\/sup> ions<\/p>\n<\/details>\n

\n

Question 18.
\nIn the diagram given below, the value of x is
\n\"MCQ
\n(a) 0.35 V
\n(b) 0.65 V
\n(c) 0.325 V
\n(d) -0.65 V<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) 0.325 V<\/p>\n<\/details>\n

\n

Question 19.
\nBy how much will the potential of a zinc electrode change if the solution of ZnSO4<\/sub> in which it is immersed is diluted to 10 times at 298 K?
\n(a) Decreases by 30 mV
\n(b) Increases by 30 mV
\n(c) Increases by 60 mV
\n(d) Decreases by 60 mV<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Increases by 30 mV<\/p>\n<\/details>\n

\n

Question 20.
\nThe e.m.f. of the cell:
\nCu(s) | Cu2+<\/sup> (1M) | | Ag+<\/sup> (1M) | Ag is 0.46 V. The standard reduction potential of Ag+<\/sup>|Ag is 0.80 V. The standard reduction potential of Cu2+<\/sup> |Cu is
\n(a) -0.34 V
\n(b) 1.26 V
\n(c) -1.26 V
\n(d) 0.34 V<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) 0.34 V<\/p>\n<\/details>\n

\n

Question 21.
\nSaturated solution of KNO3<\/sub> is used to make salt bridge because
\n(a) velocity of K+<\/sup> is greater than that of NO\\(_3^-\\)
\n(b) velocity of NO\\(_3^-\\) is greater than that of K+<\/sup>
\n(c) velocity of both K+ and NO\\(_3^-\\) are nearly the same
\n(d) KNO3<\/sub> is highly soluble in water.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) velocity of both K+ and NO\\(_3^-\\) are nearly the same<\/p>\n<\/details>\n

\n

Question 22.
\nAluminium displaces hydrogen from acids, but copper does not. A galvanic cell prepared by combining Cu\/Cu2+<\/sup> and Al\/Al3+<\/sup> has an emf of 2.0 V at 298 K. If the potential of copper electrode is + 0.34 V, that of aluminium electrode is
\n(a) -2.3 V
\n(b) +2.34 V
\n(c) -1.66 V
\n(d) 1.66 V<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) -1.66 V<\/p>\n<\/details>\n

\n

Question 23.
\nStandard electrode potentials are:
\nFe2+<\/sup>\/Fe (E\u00b0= -0.44 V), Fe3+<\/sup>\/Fe2+<\/sup> (E\u00b0 = 0.77 V)
\nFe2+<\/sup>, Fe3+<\/sup> and Fe blocks are kept together, then
\n(a) Fe3+<\/sup> increases
\n(b) Fe3+<\/sup> decreases
\n(c) Fe2+<\/sup> |Fe3+<\/sup> remains unchanged
\n(d) Fe2+<\/sup> decreases<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Fe3+<\/sup> decreases<\/p>\n<\/details>\n

\n

Question 24.
\nThe standard reduction potentials for two reactions are given below:
\nAgCl(s) + e–<\/sup> \u2192 Ag(s) + Cl–<\/sup>(aq) E\u00b0 = 0.22 V
\nAg+<\/sup>(aq) + e–<\/sup> \u2192 Ag(s) E \u00b0 = 0.80 V
\nThe solubility product of AgCl under standard conditions of temperature (298 K) is given by
\n(a) 1.6 \u00d7 10-5<\/sup>
\n(b) 1.5 \u00d7 10-8<\/sup>
\n(c) 3.2 \u00d7 10-10<\/sup>
\n(d) 1.5 \u00d7 10-10<\/sup><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) 1.5 \u00d7 10-10<\/sup><\/p>\n<\/details>\n

\n

Question 25.
\nThe e.m.f. of the following Daniell cell at 298 K is E1<\/sub>
\nIn | ZnSO4<\/sub> (0.01 M) | | CuSO4<\/sub> (1.0) | Cu
\nWhen concentration of ZnSO4<\/sub> is 1.0 M and that of CuSO4<\/sub> is 0.01 M, the e.m.f. changed to E2<\/sub>. What is the relationship between E1<\/sub> and E2<\/sub>?
\n(a) E1<\/sub> > E2<\/sub>
\n(b) E1<\/sub> < E2<\/sub>
\n(c) E1<\/sub> = E2<\/sub>
\n(d) E2<\/sub> = 0 \u2260 E1<\/sub><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) E1<\/sub> > E2<\/sub><\/p>\n<\/details>\n

\n

Question 26.
\nE\u00b0Cu2+<\/sup>\/cu<\/sub> = 0.34 V and E\u00b0Zn2+<\/sup>\/Zn<\/sub> = -0.76 V. A Daniell cell contains 0.1 M ZnSO4<\/sub> solution and 0.01 M CuSO4<\/sub> solution at its electrodes. The EMF of the cell is
\n(a) 1.10 V
\n(b) 1.04 V
\n(c) 1.16 V
\n(d) 1.07 V<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) 1.07 V<\/p>\n<\/details>\n

\n

Question 27.
\nConsider the following E\u0398 values E(Fe3+<\/sup>\/Fe2+<\/sup>)<\/sub> = + 0.77 V, E(Sn2+<\/sup>\/Sn)<\/sub> = -0.14 V Under standard conditions, the potential for the reaction:
\nSn(s)+2Fe3+<\/sup>(oq) \u2192 2Fe2+<\/sup>(aq) + Sn2+<\/sup>(aq)is
\n(a) 0.91 V
\n(b) 1.40 V
\n(c) 1.68 V
\n(d) 0.63 V<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 0.91 V<\/p>\n<\/details>\n

\n

Question 28.
\nIf E\u00b0(Fe2+<\/sup>\/Fe)<\/sub> = -0.441 V and E\u00b0(Fe3+<\/sup>\/Fe2+<\/sup>)<\/sub> = 0.771V, the standard E.M.F. of the reaction:
\nFe + 2Fe3+<\/sup> \u2192 3Fe2+<\/sup> will be
\n(a) 1.653 V
\n(b) 1.212 V
\n(c) 0.111 V
\n(d) 0.330 V<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) 1.212 V<\/p>\n<\/details>\n

\n

Question 29.
\nNumber of coulombs required to deposit 90 g of Al when the electrode reaction Al3+<\/sup> + 3e–<\/sup> \u2192 Al is:
\n(a) 9.65 \u00d7 104<\/sup>
\n(b) 8.685 \u00d7 105<\/sup>
\n(c) 9.65 \u00d7 105<\/sup>
\n(d) 6.955 \u00d7 104<\/sup><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) 9.65 \u00d7 105<\/sup><\/p>\n<\/details>\n

\n

Question 30.
\n10800 C of electricity through the electrolyte deposited 2.977 g of metal with atomic mass 106.4 a.m.u. The valency of metal cation is:
\n(a) 4
\n(b) 3
\n(c) 2
\n(d) 1<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 4<\/p>\n<\/details>\n

\n

Question 31.
\nThe charge on 1 gram mole ion of N3-<\/sup> is
\n(a) 6.00 \u00d7 105<\/sup> C
\n(b) 2.89 \u00d7 105<\/sup> C
\n(c) 3.98 \u00d7 105<\/sup> C
\n(d) 4.89 \u00d7 105<\/sup> C<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) 2.89 \u00d7 105<\/sup> C<\/p>\n<\/details>\n

\n

Question 32.
\nA current of 3A was passed through a solution of AuCl\\(_{ 4 }^{-}\\) ions using gold electrodes and it caused deposition of 1.234 g of Au (Atomic mass of Au = 197). The time for which the current was passed is
\n(a) 20 min 8s
\n(b) 30 min 12s
\n(c) 10 min 4s
\n(d) 10 min 40s<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) 10 min 4s<\/p>\n<\/details>\n

\n

Question 33.
\nAn electric current is passed through silver voltmeter connected to a water voltmeter. The cathode of silver voltmeter weighed 0.108 g more at the end of electrolysis. The volume of O2<\/sub> at STP evolved is
\n(a) 5.6 cm\u00b3
\n(b) 550 cm\u00b3
\n(c) 22.4 cm\u00b3
\n(d) 11.2 cm\u00b3<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 5.6 cm\u00b3<\/p>\n<\/details>\n

\n

Question 34.
\nSame amount of electric current is passed through solution of AgNO3<\/sub> and HCl. If 1.08 g of silver is obtained in the first case, the amount of hydrogen liberated at S.T.P. in the second case is:
\n(a) 112 cm\u00b3
\n(b) 22400 cm\u00b3
\n(c) 224 cm\u00b3
\n(d) 1.008 g<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 112 cm\u00b3<\/p>\n<\/details>\n

\n

Question 35.
\n4.5 g of aluminium (at. mass = 27. a.m.u) is deposited at cathode from Al3+<\/sup> solution by certain quantity of electric charge. The volume of hydrogen produced at STP from H+<\/sup> ions in solution by the same quantity of electric charge will be
\n(a) 44.8 L
\n(b) 22.4 L
\n(c) 11.2 L
\n(d) 5.6 L<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) 5.6 L<\/p>\n<\/details>\n

\n

Question 36.
\nThe quantity of electricity needed to separately electrolyse 1 M solution of ZnSO4<\/sub>, AICl3<\/sub> and AgNO3<\/sub> completely is in the ratio of
\n(a) 2 : 3 : 1
\n(b) 2 : 1 : 1
\n(c) 2 : 1 : 3
\n(d) 2 : 2 : 1<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 2 : 3 : 1<\/p>\n<\/details>\n

\n

Question 37.
\nWhen lead storage battery discharges
\n(a) SO2<\/sub> is evolved
\n(b) PbSO4<\/sub> is consumed
\n(c) Lead is formed
\n(d) H2<\/sub>SO4<\/sub> is consumed.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) H2<\/sub>SO4<\/sub> is consumed.<\/p>\n<\/details>\n

\n

Question 38.
\nIn a Leclanche dry cell, anode is:
\n(a) Graphite rod
\n(b) FeO and Fe(OH)2<\/sub>
\n(c) Zinc container
\n(d) MnO2<\/sub> + C<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Zinc container<\/p>\n<\/details>\n

\n

Question 39.
\nRust is a mixture of
\n(a) FeO and Fe(OH)3<\/sub>
\n(b) FeO and Fe(OH)2<\/sub>
\n(c) Fe2<\/sub>O3<\/sub> and Fe(OH)3<\/sub>
\n(d) Fe3<\/sub>O4<\/sub> and Fe(OH)3<\/sub>.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Fe2<\/sub>O3<\/sub> and Fe(OH)3<\/sub><\/p>\n<\/details>\n

\n

Question 40.
\nWhich of the following will be formed when lead storage battery is charged?
\n(a) Sulphuric add is consumed
\n(b) lead is consumed
\n(c) sulphuric acid is formed
\n(d) lead sulphate is formed.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) sulphuric acid is formed<\/p>\n<\/details>\n

\n

Question 41.
\nFor a H2<\/sub> – O2<\/sub> fuel cell, the theoretical voltage has been found to be 1.23V and \u0394H to be -285 kJ mol-1<\/sup>. The efficiency of the fuel cell is
\n(a) 76%
\n(b) 83%
\n(c) 89%
\n(d) 72%<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) 83%<\/p>\n<\/details>\n

\n

Question 42.
\nWhich of the following reaction occurs at cathode in H2<\/sub> – O2<\/sub> fuel cell?
\n(a) H+<\/sup> + OH–<\/sup> \u2192 H2<\/sub>O
\n(b) O2<\/sub> + 2H2<\/sub>O + 4e–<\/sup> \u2192 4 OH–<\/sup>
\n(c) 2H2<\/sub> + O2<\/sub> > 2H2<\/sub>O
\n(d) H2<\/sub> + 2OH–<\/sup> \u2192 2H2<\/sub>O + 2e–<\/sup><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) O2<\/sub> + 2H2<\/sub>O + 4e–<\/sup> \u2192 4 OH–<\/sup><\/p>\n<\/details>\n

\n

Question 43.
\nWhich of the following reaction occurs at anode during the recharging of lead storage battery?
\n(a) PbSO4<\/sub> + 2H2<\/sub>O \u2192 PbO2<\/sub> + SO\\(_{ 4 }^{2-}\\) +4H+<\/sup> + 2e–<\/sup>
\n(b) Pb + S0\\(_{ 4 }^{2-}\\) \u2192 PbSO4<\/sub> + 2e–<\/sup>
\n(c) PbSO4<\/sub> + 2e–<\/sup> \u2192 Pb + S0\\(_{ 4 }^{2-}\\)
\n(d) PbO2<\/sub> + 4H+<\/sup> + SO\\(_{ 4 }^{2-}\\) + 2e–<\/sup> \u2192 PbSO4<\/sub> + 2H2<\/sub>O<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) PbSO4<\/sub> + 2H2<\/sub>O \u2192 PbO2<\/sub> + SO\\(_{ 4 }^{2-}\\) +4H+<\/sup> + 2e–<\/sup><\/p>\n<\/details>\n

\n

Question 44.
\nIn nickel-cadmium storage cell, the electrolyte is
\n(a) moist KOH
\n(b) dil H2<\/sub>SO4<\/sub>
\n(c) aqueous NH4<\/sub>Cl
\n(d) Ni(OH)3<\/sub>(aq)<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) moist KOH<\/p>\n<\/details>\n

\n

Assertion and Reason Type Questions<\/span><\/p>\n

The questions given below consist of an assertion and a reason. Use the following key to choose the appropriate answer.
\n(a) Both Assertion (A) and Reason (R) are correct statements, and Reason (R) is the correct explanation of the Assertion (A).
\n(b) Both Assertion (A) and Reason (R) are correct statements, but Reason (R) is not the correct explanation of the Assertion (A).
\n(c) Assertion (A) is correct, Reason (R) is wrong statement.
\n(d) Assertion (A) is wrong, but Reason (R) is correct statement.<\/p>\n

Question 45.
\nAssertion: Equivalent conductance of all electrolytes decreases with increasing concentration.
\nReason: Lesser number of ions are available per gram equivalent at higher concentration.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Assertion (A) is correct, Reason (R) is wrong statement.<\/p>\n<\/details>\n

\n

Question 46.
\nAssertion: Iron is protected from corrosion by connecting magnesium metal with it. Reason: Iron acts as a cathode and magnesium as anode which gradually disappears.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) Both Assertion (A) and Reason (R) are correct statements, and Reason (R) is the correct explanation of the Assertion (A).<\/p>\n<\/details>\n

\n

Question 47.
\nAssertion: Chromium is used for coating iron.
\nReason: Chromium is non-corroding metal which forms a protective layer on iron.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) Both Assertion (A) and Reason (R) are correct statements, and Reason (R) is the correct explanation of the Assertion (A).<\/p>\n<\/details>\n

\n

Question 48.
\nAssertion: Zinc can liberate H2<\/sub> from aqueous solution of HCl.
\nReason: Zinc has +ve reduction potential.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Assertion (A) is correct, Reason (R) is wrong statement.<\/p>\n<\/details>\n

\n

Question 49.
\nAssertion: Copper sulphate solution can be kept in a zinc vessel.
\nReason: The position of zinc is higher than copper in the electrochemical series.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) Assertion (A) is wrong, but Reason (R) is correct statement.<\/p>\n<\/details>\n

\n

Question 50.
\nAssertion: For CH3<\/sub>COOH, the molar
\nconductance of 0.1 M CH3<\/sub>COOH and equivalent conductance of 0.1 N CH3<\/sub>COOH is same.
\nReason: These do not depend upon concentration.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Assertion (A) is correct, Reason (R) is wrong statement.<\/p>\n<\/details>\n

\n

Question 51.
\nAssertion: 0.1 M NH4<\/sub>OH at 25\u00b0C has more conductance than at 50\u00b0C.
\nReason: Conductance of a weak electrolyte increases with increase in temperature.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) Assertion (A) is wrong, but Reason (R) is correct statement.<\/p>\n<\/details>\n

\n

Hope the information shared regarding the NCERT MCQ Questions for Class 12 Chemistry Chapter 3 Electrochemistry with Answers Pdf free download is true and genuine as far as our knowledge is concerned. If you feel any information regarding CBSE Class 12 Chemistry Electrochemistry MCQs Multiple Choice Questions with Answers is missing do reach us and we will look into it and add it accordingly.<\/p>\n","protected":false},"excerpt":{"rendered":"

Students are advised to practice the NCERT MCQ Questions for Class 12 Chemistry Chapter 3 Electrochemistry with Answers Pdf free download is available here. MCQ Questions for Class 12 Chemistry with Answers are prepared as per the Latest Exam Pattern. Students can solve these Electrochemistry Class 12 MCQs Questions with Answers and assess their preparation …<\/p>\n

MCQ Questions for Class 12 Chemistry Chapter 3 Electrochemistry with Answers<\/span> Read More »<\/a><\/p>\n","protected":false},"author":9,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"spay_email":""},"categories":[35],"tags":[],"yoast_head":"\nMCQ Questions for Class 12 Chemistry Chapter 3 Electrochemistry with Answers - NCERT Solutions<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/ncertsolutions.guru\/mcq-questions-for-class-12-chemistry-chapter-3\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"MCQ Questions for Class 12 Chemistry Chapter 3 Electrochemistry with Answers - NCERT Solutions\" \/>\n<meta property=\"og:description\" content=\"Students are advised to practice the NCERT MCQ Questions for Class 12 Chemistry Chapter 3 Electrochemistry with Answers Pdf free download is available here. 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