JEE Questions for Chemistry Electrochemistry Quiz 8 - MCQExams.com

The resistance of 0.01N solution of an electrolyte AB at 328 K is 100 ohm. The specific conductance of solution is (cell constant = 1 cm-1)
  • 100 ohm
  • 10-2 ohm–1
  • 10-2 ohm-1 cm-1
  • 102 ohm -cm
What weight of copper will be deposited by passing 2 faradays of electricity through a cupric salt (At. wt. of Cu= 63.5)?
  • 2.0 g
  • 3.175g
  • 63.5g
  • 127.0g
2.5 faraday of electricity is passed through a solution of CuSO4.The number of gram equivalent of copper deposited on the cathode will be
  • 1
  • 2
  • 2.5
  • 1.25
A solution of CuSO4 is electrolysed for 7 minutes with a current of 0.6 ampere. The amount of electricity passed is equal to
  • 4.2 columbs
  • 2.6 × 10-3 Faraday
  • 126 Coulombs
  • 35 Coulombs
From the solution of an electrolyte, one mole of electron will deposit at cathode.
  • 63.5 gm of Cu
  • 24 gm of Mg
  • 11.5 gm of Na
  • 9.0 gm of Al
When an electric current is passed through acidulated water, 112 ml of hydrogen gas at NTP is collected at the cathode in 965 seconds.The current passed in amperes, is
  • 1.0
  • 0.5
  • 0.1
  • 2.0
The charge required to librerate 11.5 g sodium from fused sodium chloride is
  • 0.5 faraday
  • 1.0 faraday
  • 1.5 faraday
  • 96500 coulombs
How long will it take for a current of 3 amperes to decompose 36 g of water ? ( Eq. wt of hydrogen is 1 and that of oxygen 8)
  • 36 hours
  • 18 hours
  • 9 hours
  • 4.5 hours
What is the amount of chlorine evolved when 2 amperes of current is passed for 30 minutes in an aqueous solution of NaCl ?
  • 66 g
  • 1.32 g
  • 33 g
  • 99 g
The same amount of electricity was passed through two separate electrolytic cells containing solutions of nickel nitrate and chromium nitrate respectively. If 0.3 g of nickel was deposited in the first cell, the amount of chromium deposited is (At wt. Ni = 59, Cr = 52)
  • 0.1 g
  • 0.17 g
  • 0.3 g
  • 0.6 g
How much quanitity of electricity has to be passed through 200 ml of 0.5 M CuSO4 solution to completely deposit copper
  • 96500 C
  • 2 × 9650C
  • 2 × 96500C
  • 4 × 96500C
Time required to deposit one millimole of aluminium metal by the passage of 9.65 amperes through aqueous solution of aluminium ions is
  • 30 s
  • 10 s
  • 30,000s
  • 10,000 s

Chemistry-Electrochemistry-3356.png
  • – 0.35 V
  • 0.35 V
  • 1.17 V
  • – 1.17 V
The standard reduction potential for Fe2+/Fe and Sn2+/Sn electrodes are ‒ 0.44 and ‒ 0.14 volt respectively. For the cell reaction : Fe2+ + Sn → Fe + Sn2+, the standard emf is
  • + 0.30 V
  • ‒ 0.58 V
  • +0.58 V
  • ‒ 0.30 V

Chemistry-Electrochemistry-3359.png
  • + 0.07 V
  • ‒ 0.07 V
  • + 0.77 V
  • ‒ 0.77 V

Chemistry-Electrochemistry-3361.png
  • 0.54 V
  • ‒ 0.54 V
  • + 0.18 V
  • ‒ 0.18 V.
The emf of the cell H2 (1 atm) Pt |H+ (a = x) ||H2 (1atm)pt at 25oC is 0.59 V. The pH of the solution is
  • 1
  • 4
  • 7
  • 10
If the standard electrode potential of Cu2+/Cu electrode is 0.34 V, what is the electrode potential of 0.01 M concentration of Cu2+ ? (T= 298 K)
  • 0.399 V
  • 0.281 V
  • 0.222V
  • 0.176 V
The specific conductances of four electrolytes in ohm-1 cm-1 are given below. Which one offers higher resitance to the passage of electric current?
  • 7.0 × 10-5
  • 9.2 × 10-9
  • 6.0 × 10-7
  • 4.0 × 10-8
The equivalent conductances at infinite dilution (^0) for electrolyte BA and CA are 140 and 120 S cm2 eq-1. The equivalent conductance at infinite dilution for BX is 198 S cm2 eq-1. The ^0 (in S cm2 eq-1 ) of CX is
  • 178
  • 198
  • 218
  • 130
A current of 12 ampere is passed through an electrolytic cell containing aq. NiSO4 solution. Both Ni and H2 gas are formed at the cathode. The current efficiency is 60%. What is the mass of nickel deposited on the cathode per hour ? (At. wt. of Ni = 98 .
  • 7.883 gm
  • 3.941 gm
  • 5.91 gm
  • 2.645 gm
Resistance of 0.2 M solution of an electrolyte is 50Ω. The specific conductance of the solution is 1.3 Sm-1. If resistance of the 0.4 M solution of the same electrolyte is 260Ω, its molar conductivity is
  • 6250 Sm2 mol-1
  • 6.25 × 10-4 Sm2 mol-1
  • 625 × 10-4 Sm2 mol-1
  • 62.5 Sm2 mol-1
Suppose that gold is being plated on to another metal in an electrolytic cell. The half reaction producing the Au (s) is
AuCl‒4 → Au(s) + 4Cl‒ ‒ 3e‒
If a 0.30 A current run for 15 min, what mass of Au(s) will be plated, assuming all the electrons are used in the reduction of AuCl‒4? The Faraday constant is 96485 c/mol and molar mass of Au is 197.
  • 0.184 g Au
  • 0.551 g Au
  • 1.84 g Au
  • 0.613 g Au
Aluminium oxide may be electrolysed at 1000°C to furnish aluminium metal (atomic mass = 27 u; 1F = 96500 C). The cathode reaction is
Al 3+ + 3e‒ → Al0
To prepare 5.12 kg of aluminium metal by this method would require
  • 5.49 × 101 C of electricity
  • 5.49 × 104 C of electricity
  • 1.83 × 107 C of electricity
  • 5.49 × 107 C of electricity
In a galvanic cell, the salt bridge
  • does not participate chemically in the cell reaction
  • stops the diffusion of ions from one electrode to another
  • is necessary for the occurrence of the cell reaction
  • ensure moving of the two electrolyte solution
The standard reduction potential data at 25oC is given below
Eo(Fe3+/Fe2+) = 0.77V
Eo(Fe2+/Fe) = -0.44V
Eo(Cu2+?Cu) = + 0.34 V
Eo(Cu+/Cu) = + 0.52 V
Eo (O2(g) + 4H+ + 4e-→2H2O) = 1.23 V
Eo (O2 (g) + 2H2O + 4e- →4OH-) = + 0.40 V
Eo (Cr3+/Cr) = -0.74 V;
Eo(Cr2+/Cr) = -0.91 V
Match Eo of the redox pair in List I with the values given in List II and select the correct answer using the codes given below the lists
Chemistry-Electrochemistry-3370.png
  • P = 4, Q = 1, R = 2, S = 3
  • P = 2, Q = 3, R = 4, S = 1
  • P = 1, Q = 2, R = 3, S = 4
  • P = 3, Q = 4, R = 1, S = 2
The standard reduction potential for Zn2+/Zn, Ni2+ /Ni and Fe2+/Fe are - 0.76, - 0.23 and - 0.44 V respectively. The reaction X + Y 2+ → X 2+ + Y will be spontaneous when
  • X = Ni, Y = Fe
  • X = Ni, Y = Zn
  • X = Fe, Y = Zn
  • X = Zn, Y = Ni

Chemistry-Electrochemistry-3371.png
  • – 1.08 volts
  • – 0.40 volts
  • 1.08 volts
  • 2.50 Volts
The standard oxidation potential of zinc and silver in water at 298 K are
Zn(s) → Zn2+ + 2e–, E = 0.76V, Ag(s) → Ag+ + e–, E = –0.80V
which of the following reactions actually takes place?
  • Zn(s) + 2Ag+(aq) → Zn2+(aq) + 2Ag(s)
  • Zn2+ + 2Ag(s) → 2Ag+(s) + Zn(s)
  • Zn(s) + Ag(s) → Zn2+(aq) + Ag+(aq)
  • Zn2+(aq) + Ag+(aq) → Zn(s) + Ag(s)
The electric charge for electrode deposition of one gram equivalent of substance is
  • one ampere for one second
  • 956500 coulombs per second
  • charge on one mole of electrons
  • one ampere for one hour
0:0:1


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