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>\nElectrochemistry 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>\nAnswer: (a) 1<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (b) ohm-1<\/sup> cm-1<\/sup><\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (c) 46<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (a) 280 S cm\u00b2 mol-1<\/sup><\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (a) 1.06 \u00d7 10\u00b2<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (c) 128 S cm\u00b2 mol-1<\/sup><\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (c) 388.8 ohm-1<\/sup> cm\u00b2 gm eq-1<\/sup><\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (b) 0.02<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (d) 2.5 \u00d7 10-4<\/sup><\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (b) 392<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (d) Cell can work indefinitely.<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (b) Zinc acts as anode and copper as cathode.<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (a) 0.637 V<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (a) – 0.81 V<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (c) E = E\u00b0 + \\(\\frac { RT }{nF}\\) ln [Mn+<\/sup>]<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (c) \u0394G\u00b0 = -nF E\u00b0cell<\/sub><\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (b) increase in the concentration of Sn2+<\/sup> ions<\/p>\n<\/details>\n
\nQuestion 18.
\nIn the diagram given below, the value of x is
\n
\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>\nAnswer: (c) 0.325 V<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (b) Increases by 30 mV<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (d) 0.34 V<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (c) velocity of both K+ and NO\\(_3^-\\) are nearly the same<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (c) -1.66 V<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (b) Fe3+<\/sup> decreases<\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (d) 1.5 \u00d7 10-10<\/sup><\/p>\n<\/details>\n
\nQuestion 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>\nAnswer: (a) E1<\/sub> > E2<\/sub><\/p>\n<\/details>\n
\nQuestion 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\n