JEE Questions for Chemistry Electrochemistry Quiz 3 - MCQExams.com

When Cu reacts with AgNO3 solution, the reaction takes place is
  • oxidation of Cu
  • reduction of Cu
  • oxidation of Ag
  • reduction of NO3
Which will reduce zinc oxide to zinc?
  • Mg
  • Pb
  • Cu
  • Fe
The metal that does not displace hydrogen from an acid is
  • Ca
  • Al
  • Zn
  • Hg
Which of the following ions can be replaced by H+ ions when H2 gas is bubbled through the solutions containing these ions?
  • Li+
  • Ba2+
  • Cu2+
  • Be2+
H2 cannot be displaced by
  • Li+
  • Sr2+
  • Al3+
  • Ag+

Chemistry-Electrochemistry-3262.png
  • +1.10 V
  • -1.10 V
  • +0.42 V
  • -0.42 V
The standard electrode potentials of Ag+ / Ag is + 0.80V and Cu+/Cu is + 0.34 V. These electrodes are connected through a salt bridge and if
  • copper electrode acts as a cathode, then Eocell is +0.46 V
  • silver electrode acts as anode, then Eocell is -0.34 V
  • copper electrode acts as anode, then Eocell is +0.46 V
  • silver electrode acts as a cathode, then Eocell is -0.34 V
  • silver electrode acts as anode and Eocell is +1.14 V
For cell reaction, Zn + Cu2+ → Zn2+ + Cu
  • Zn|Zn2+||Cu2+|Cu
  • Cu|Cu2+||Zn2+|Zn
  • Cu|Zn2+||Zn|Cu2+
  • Cu2+|Zn||Zn2+|Cu
For the following cell with hydrogen electrodes at two different pressures p1 and p2
Pt(H2)|H+ (aq)|Pt(H2) emf is given by

  • Chemistry-Electrochemistry-3263.png
  • 2)
    Chemistry-Electrochemistry-3264.png

  • Chemistry-Electrochemistry-3265.png

  • Chemistry-Electrochemistry-3266.png
For a cell given below,
Ag|Ag+||Cu2+|Cu
Ag+ + e- → Ag, Eo = x
Cu2+ + 2e- → Cu, Eo = y Eocell is
  • x + 2y
  • 2x + y
  • y - x
  • y - 2x
For hydrogen-oxygen fuel cell at 1atm and 298 K
H2 (g) = 1/2 O2 → H2O(l), ∆G = -240KJ
Eo for the cell is approximately (Given, F = 96500C)
  • 2.48 V
  • 1.25 V
  • 2.5 V
  • 1.24 V
Which of the following reactions cannot be electrochemical cell?
  • H2 + O2 → H2O
  • AgNO3 + Zn → Zn(NO3)2 + Ag
  • AgNO3 + NaCl → AgCl ↓ + NaNO2
  • KMnO4 + FeSO4 + H2SO4 →K2SO4 + Fe2(SO4)3 + MnSO4 + H2O
In a galvanic cell, the electrons flow from
  • anode to cathode through the solution
  • cathode to anode through the solution
  • anode to cathode through the external circuit
  • cathode to anode through the external circuit
What is the cell reaction occurring in Daniel cell (Galvanic cell) ?
  • Cu(s) + ZnSO4 (aq) → CuSO4 (aq) + Zn (s)
  • Zn(s) + CuSO4 (aq) → Cu(s) + ZnSO4 (aq)
  • Ni(s) + ZnSO4 (aq) → NiSO4 (aq) + Zn(s)
  • 2Na(s) + CdSO4 (aq) → Na2SO4 (aq) + Cd(s)
A galvanic cell is constructed using the redox reaction,
1/2 H2 (g) + AgCl (s) ⇌ H+ (aq) + Cl- (aq) + Ag(s)
it is represented as
  • Pt|H2 (g)|HCl solution ||AgNO3 solution| Ag
  • Ag|AgCl(s)|KCl solution||HCl solution, H2(g)|Pt
  • Pt|H2(g)|KCl solution || AgCl(s)|Ag
  • Pt|H2 (g), HCl solution|| AgCl(s)| Ag
Stainless steel does not rust because
  • chromium and nickel combine with iron
  • chromium forms an oxide layer and protects iron from rusting
  • nickel present in it, does not rust
  • iron forms a hard chemical compound with chromium present in it
Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are
  • Fe is oxidised to Fe2+ and dissolved oxygen in water is reduced to OH-
  • Fe is oxidised to Fe3+ and H2O is reduced to O2-2
  • Fe is oxidised to Fe2+ and H2O is reduced to O-2
  • Fe is oxidised to Fe2+ and H2O is reduced to O2
When electric current is passed through acidified water for 1930 s, 1120 mL, of H2 gas is collected (at STP) at the cathode. What is the current passed in amperes?
  • 0.05
  • 0.50
  • 5.0
  • 50
Of the following metals that cannot be obtained by electrolysis of the aqueous solution of their salts are
  • Ag and Mg
  • Ag and Al
  • Mg and Al
  • Cu and Cr.
The equivalent conductivity of a solution containing 2.54g of CuSO4 per L is 91.0 ω-1 cm2 eq-1. Its conductivity would be
  • 2.9 × 10-3 Ω-1 cm-1
  • 1.8 × 10-2 Ω-1 cm-1
  • 2.4 × 10-4 Ω-1 cm-1
  • 3.6 × 10-3 Ω-1 cm-1

Chemistry-Electrochemistry-3270.png
  • 275.6, 091
  • 275.6, 9.1
  • 266.6, 9.6
  • 30, 84
Ionic mobility of which of the following alkali metal ions is lowest when aqueous solution of their salts are put under an electric field ?
  • K
  • Rb
  • Li
  • Na
The ionic conductance of Ba2+ and Cl- are respectively 127 and 76Ω- cm2 as infinite dilution. The equivalent conductance (in Ω-1 cm2) of BaCl2 at infinite dilution will be
  • 330
  • 203
  • 139.5
  • 51
AgNO3 (aq) was added to an aqueous KCl solution gradually and the conductivity of the solution was measured. The plot of conductance (˄) versus the volume of AgNO3 is
Chemistry-Electrochemistry-3273.png
  • (I)
  • (II)
  • (III)
  • (IV)
By diluting a weak electrolyte, specific conductivity (KC) and equivalent conductivity (λC) change as
  • Both increase
  • KC increases, λC decreases
  • KC decreases, λC increases
  • Both decreases
The resistance of N/10 solution is found to be 2.5 × 103Ω. The equivalent conductance of the solution is (cell constant = 1.25 cm-1)
  • 2.5Ω-1 cm2 equiv-1
  • 5.0Ω-1 cm2 equiv-1
  • 2.5Ω-1 cm-2 equiv-1
  • 5.0Ω-1 cm-2 equiv-1
The value of Ʌ∞eq for NH4 Cl, NaOH and NaCl are respectively, 149.74, 248.1 and 126.4 Ω-1 cm2 equiv-1. The value of Ʌ∞eq of NH4OH is
  • 371.44
  • 271.44
  • 71.44
  • Cannot be predicated from given data
The specific conductivity of 0.1 N KC1 solution is 0.0129 Ω-1 cm-1 . The resistance of the solution in the cell is 100 Ω. The cell constant of the cell will be
  • 1.10
  • 1.29
  • 0.56
  • 2.80
If the molar conductance values of Ca2+ and Cl- at infinite dilution are respectively 118.88 × 10-4 m2 mho mol-1 and 77. 33 × 10-4 m2 mho mol-1 then that of CaCl2 is (in m2 mho mol-1)
  • 118.88 × 10-4
  • 154.66 × 10-4
  • 273.54 × 10-4
  • 196.21 × 10-4
The limiting molar conductivities Ʌo for NaCl , KBr and KCl are 126, 152 and 150 S cm2 mol-1 respectively. The Ʌo for NaBr is
  • 128 S cm2 mol-1
  • 176 S cm2 mol-1
  • 278 S cm2 mol-1
  • 302 S cm2 mol-1
0:0:1


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