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221. The reaction ½ H2(g) + AgCl (s) ↔ H+(aq) + Cl- (aq) + Ag(s) galvanic cell is a) Ag | AgCl (s) | KCl (soln) || HCl (soln), H2(g) | Pt b) Pt | H2(g) | HCl (soln) || AgNO3 (soln) | Ag (c) Pt | H2(g) | HCl (soln) | AgCl (s) | Ag. d) Pt | H2(g) | KCl (soln) || AgCl (s) | Ag
c) Zn(s) + Ag(s) → Zn2+ (aq) + Ag+ (aq) d) Zn2+ (aq) + Ag+ (aq) → Zn(s) + Ag(s) 225. Copper cannot liberate H2 from dilute acids because a) Hydrogen is below Cu in the electrochemical series b) Copper is a coinage metal (c) Copper has higher reduction potential than H2 d) Copper is a transition metal
a) -2.10V b) +2.10V (c) 1.22V d) -1.22V 227. At constant temperature, a graph of reduction potential along y-axis, logarithm of concentration of metal ion along x-axis is a) Straight line with a negative slope b) Straight line passing through the origin (c) Straight line of intercept E0. d) A curve
c) K+ and Cl- ions have same velocity d) It is ionic 229.  = -1.7V and  = -0.44V. E.M.F. If a cell is constructed by combining them
a) Aluminium is cathode (b) Iron is cathode c) Electrons flow from iron to aluminium externally d) Iron gradually gets dissolved
a) 1 b) 2 c) 1.018 (d) 0 231. At 298 K electrode potentials of a hydrogen electrode containing HCl of pH 2.2 is a) 0 V b) 2.2 V (c) -0.132V d) +0.132V 232. Al displaces H2 from dilute acids but Cu does not. A cell prepared by combining Cu | Cu+2 and Al | Al+3 has an e.m.f. of 2 volts. If the electrode potential of Cu is +0.34 volt, that of Al is a) 2.34 V b) 1.66 V (c) -1.66 V d) -2.34 V 233. S.H.E. employs ‘platinised’ platinum because a) It prevents corrosion of platinum (b) It helps more efficient adsorption by the surface c) It prevents reaction of the metal with HCl d) Powdered platinum is very inert
a) A is readily reduced (b) A is readily oxidized c) A- is readily reduced d) A- is readily oxidized
a) A (b) B c) C d) D 237. A metal which does not liberate H2 from dilute acids is dipped into a salt solution. This electrode is attached to Al | Al+3 electrode. The resulting cell e.m.f. is 2.46 V. If the electrode potential of Al -1.66 V, that of the metal electrode is a) -0.8 V b) 4.10 V (c) +0.8 V d) None of these 238. A hydrogen electrode contains HCl solution of pH 3 at 298K. Its electrode potential is a) +0.18 V (b) -0.18 V c) 3.8 V d) 3.8/0.0591 239. Two copper wires are separately dipped in 0.1M CuSO4 and 0.01M CuSO4 solutions at 298K. These two electrodes are combined to form a cell whose e.m.f. is a) 0.34 V b) 0.34 + 240. A hydrogen electrode has an electrode potential of -0.24 V at 298 K. pH of solution is a) 6 (b) 4 c) 2.2 d) 3.3 241. The standard reduction potential of Fe+2 | Fe and Cu2+ | Cu electrodes are -0.44 V and +0.34 V respectively. Which one of the following statements is true? (a) Fe will reduce Cu2+ ions b) Fe will oxidise Cu c) Cu will reduced Fe2+ ions d) Cu2+ ion will reduce Fe2+ ions 242. Which among the following is the strongest reducing agent? a) Cr(s) b) Fe(s) (c) Zn(s) d) H2(g) 243. In a reaction between zinc and iodine in which zinc iodide is formed, what is being oxidized? a) Zn ions b) Iodide ions (c) Zn atom d) Iodine 244. A metal ion M3+ after loss of three electrons in a reaction will have an oxidation number equal to a) 0 b) +2 c) +3 (d) +6 245. Specific conductance of 0.02 M KCl is 0.0022 Scm-1, its molar conductance is a) 44 (b) 110 c) 0.11 d) 9.09 246.Equivalent conductance of 0.01 M HCl is 400 ×10-4 Sm2 / gram eq. mass. Its specific conductance is a) 400 b) 40 (c) 0.4 d) 4 247. For BaCl2 a) Molar conductance = equivalent conductance b) 2 × molar conductance = equivalent conductance (c) Molar conductance = 2 × equivalent conductance d) Molar conductance = 2 × specific conductance
a) Molar conductance = equivalent conductance (b) Molar conductance = 2 × equivalent conductance c) Equivalent conductance = 2 × molar conductance d) None 250. The best conductor of electricity below in a 1M solution of a) Boric acid b) Acetic acid (c) Sulphuric acid d) Phosphoric acid 251. The unit of equivalent conductivity is [C.P.M.T. 99] a) ohm cm (b) Ohm-1 cm+2 (gram equivalent)-1 c) Ohm cm2 (g equivalent)-1 d) S cm-2
(a) 1.06×102 b) 1.06×103 [Kerala MEE 2001] c) 1.06×104 d) 5.3×102
a) 1.26×10-5 (b) 1.26×10-3 c) 1.26×10-4 d) 0.0063 254. Molar ionic conductivities of a bivalent electrolyte are 57 and 73. The molar conductivity of the solution will be [D.M.P.T.2002] (a) 130 S cm2 mol-1 b) 65 S cm2 mol-1 c) 260 S cm2 mol-1 d) 187 S cm2 mol-1 a 255. The equivalent conductivity of 0.1M weak acid is 100 times less than that of infinite dilution. The degree of dissociation is a) 100 b) 10 (c) 0.01 d) 0.001 [Tamil Nadu CET 2001, 02] 256. What weight of copper will be deposited by passing 2 faradays of electricity through a cupric salt solution? (At. Mass of Cu = 63.5) a) 2.0 g b) 175 g (c) 63.5 g d) 127.0 g [NCERT] 257.On the electrolysis of aqueous solution of sodium sulphate, on cathode we get a) Na (b) H2 c) SO2 d) SO3 258. On electrolyzing a solution of dilute H2SO4 between platinum electrodes, the gas evolved at the anode is [C.B.S.E. 1992] a) SO3 b) SO2 (c) O2 d) H2 259.One faraday of electricity will liberate one gram atom of the metal from a solution of a) AuCl3 b) BaCl2 c) CuSO4 (d) NaCl 260. The charge required to liberate 11.5 g of sodium is [A.I.I.M.S.1992] (a) 0.5 Faraday b) 1.0 Faraday c) 1.5 Faraday d) 96500 coulomb 261. Four moles of electrons were transferred from anode to cathode in an experiment on electrolysis of water. The total volume of the two gases (dry at STP) produced will be approximately (in litres) a) 22.4 b) 44.8 (c) 67.2 d) 89.4 [A.I.I.M.S. 1993] --- Questions for practice Directory: doc doc -> Enterprise Network Management iPost: Implementing Continuous Risk Monitoring at the Department of State doc -> Concept stage doc -> Application for acem doc -> What programs are available? doc -> 100 Village Primary School Music Classrooms doc -> Observational Assessment of Teaching Practices Teaching Assessment Initiative Proposal Submitted to The Teachers for a New Era project doc -> Concept stage doc -> Traditional British values Download 230.37 Kb. Share with your friends:
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(c) 
d) 0.0295 V