JEE Questions for Chemistry Electrochemistry Quiz 2 - MCQExams.com

A lamp draws a current of 1.0 A. Find the charge in coulomb used by the lamp in 60 s.
  • 0.6 C
  • 60 C
  • 600 C
  • 0.006 C
The charge required to liberate one gram equivalent of an element is
  • 96500 F
  • 1 F
  • 1 C
  • None of these
In the electrolysis of water, 1 F of electrical energy would evolve
  • 1 mole of oxygen
  • 1 g atom of oxygen
  • 8 g of oxygen
  • 22.4 L of oxygen
Same amount of electric current is passed through solutions of AgNO3 and HCl . If 1.08 g of silver is obtained in the first case, the amount of hydrogen liberated at STP in the second case is
  • 224cm3
  • 1.008 g
  • 112 cm3
  • 22400cm3
When electric current is passed through an ionic hydride in molten state
  • hydrogen is liberated at anode
  • hydrogen is liberated at cathode
  • no change takes place
  • hydride ion migrates towards cathode
  • hydride ion remains in solution
On passing 0.5 F of electricity through molten sodium chloride, sodium deposited at cathode will be
  • 29.25 g
  • 11.50 g
  • 58.50 g
  • 0.00 g
Calculate the volume of H2 gas at NTP obtained by passing 4 A through acidified H2O for 30 min is
  • 0.0836 L
  • 0.0432 L
  • 0.1672 L
  • 0.836 L
The charge required for reduction of 1 mole o f Cr2 O2-7 ions to Cr3+ is
  • 96500C
  • 2 × 96500 C
  • 3 × 96500 C
  • 6 × 96500 C
The standard emf for the cell reaction
2Cu+ (aq) → Cu(s) + Cu2+ (aq)
is + 0.36 V at 298 K. The equilibrium constant of the reaction is
  • 5 × 106
  • 1.4 × 1012
  • 7.4 × 1012
  • 1.2 × 106
Given that; Zn2+ / Zn = -0.762 V, Mg2+ / Mg = - 2.37V. Then, Zn + MgCl2 → ?
  • ZnCl2 + Mg
  • ZnCl2 + MgCl2
  • Zn + Mg
  • No reaction
The standard emf of a cell involving one electron change is found to be 0.591 V at 25°C. The equilibrium constant of the reaction is (F = 96500 C mol-1)
  • 1.0 × 101
  • 1.0 × 105
  • 1.0 × 1010
  • 1.0 × 1030
Eo values of Mg2+ / Mg is -2.37 V of Zn2+ / Zn is -0.76 V and Fe2+ / Fe is -0.44 V.
Which of the statements is correct ?
  • Zn will reduce Fe2+
  • Zn will reduce Mg2+
  • Mg oxidises Fe
  • Zn oxidises Fe
If the standard electrode potential of Cu2+ / Cu electrode is 0.34 V, What is the electrode potential at 0.01 M concentration of Cu2+ ?
(T = 298 K)
  • 0.399 V
  • 0.281 V
  • 0.222 V
  • 0.176 V
In which of the following pairs, the constants/ quantities are not mathematically related to each other?
  • Gibbs free energy and standard cell potential
  • Equilibrium constant and standard cell potential
  • Rate constant and activation energy
  • Rate constant and standard cell potential
Dipping iron article into a strongly alkaline solution of sodium phosphate
  • does not affect the article
  • forms Fe2O3 ∙ x H2O on the surface
  • forms iron phosphate film
  • forms ferric hydroxide
Cu+ (aq) is unstable in solution and undergoes simultaneous oxidation and reduction, according to the reaction 2Cu+ (aq) ⇌ Cu2+ (aq) + Cu (s)
Choose correct Eo for the above reaction, if
Chemistry-Electrochemistry-3255.png
  • -0.38 V
  • +0.49 V
  • +0.38 V
  • -0.19 V
The cell reaction is spontaneous, when
  • Eored is negative
  • Eored is positive
  • ∆Go is negative
  • ∆Go is positive
Hydrogen gas is not liberated when the following metal is added to dil. HCl
  • Ag
  • Zn
  • Mg
  • Sn
The cell reaction of the galvanic cell Cu(s) | Cu2+ (aq) || Hg2+ (aq) | Hg (l ) is
  • Hg + Cu2+ → Hg2+ + Cu
  • Hg + Cu2+ → Cu+ + Hg+
  • Cu + Hg → CuHg
  • Cu + Hg2+ → Cu2+ + Hg
Which one of the following condition will increase the voltage of the cell represented by the equation?
Cu(s) + 2Ag+ (aq) ⇌ Cu2+ (aq) + 2Ag(s)
  • Increase in the dimension of Cu electrode
  • Increase in the dimension of Ag electrode
  • Increase in the concentration of Cu2+ ions
  • Increase in the concentration of Ag+ ions
The standard emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25C°. The equilibrium constant of the reaction would be
(Given, F = 96500 C mol-1, R = 8. 314 JK-1 mol-1 )
  • 2.0 × 1011
  • 4.0 × 1012
  • 1.0 × 102
  • 1.0 × 1010
An alloy of Pb-Ag weighing 1.08 g was dissolved in dilute HNO3 and the volume made to 100 mL. A silver electrode was dipped in the solution and the emf of the cell set-up Pt (s), H2 (g) | H+ (1 M) || Ag+ (aq) | Ag(s) was 0.62 V. If E°cell = 0.80 V , what is the percentage of Ag in the alloy ? (At 25oC, RT/F = 0.06)
  • 25
  • 2.50
  • 10
  • 1
  • 50
The cell reaction of a cell is
Mg (s) + Cu2+ (aq) → Cu(s) + Mg2+ (aq). If the standard reduction potentials of Mg and Cu are - 2.37 and + 0.34 V respectively. The emf of the cell is
  • 2.03 V
  • -2.03 V
  • +2.71 V
  • -2.71 V
Sn4+ + 2e- → Sn2+, Eo = 0.13V
Br2 + 2e- → 2 Br-, Eo = 1.08 V
Calculate Keq for the cell reaction for the cell formed by two electrodes.
  • 1041
  • 1032
  • 10-32
  • 10-42
The standard electrode potential of hydrogen electrode at 1 M concentration and hydrogen gas at 1 atm pressure is
  • 1 V
  • 6 V
  • 8 V
  • 0 V

Chemistry-Electrochemistry-3258.png
  • 6.26 × 10-7
  • 5.33 × 10-4
  • 6.26 × 107
  • 5.33 × 104

Chemistry-Electrochemistry-3259.png
  • 1.68 V
  • 1.40 V
  • 0.91 V
  • 0.63 V
If the H+ concentration decreased from 1 M to 10-4 M at 25oC for the couple MnO-4/ Mn2+, then the oxidisting power of the MnO-4/ Mn2+ couple decreases by
  • -0.18 V
  • 0.18 v
  • 0.38 V
  • -0.38 V
Reduction potentials of A, B ,C and D are 0.8 V, 0.79 V, 0.34 V and - 2.37 V respectively. Which element displaces all the other three elements?
  • B
  • A
  • D
  • C
Calculate the equilibrium constant for the reaction, at 25oC
Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s)
at 25oC, Eocell = 0.47 V, R = 8.134 JK-1 F = 96500 C is
  • 1.8 × 1015
  • 8.5 × 1015
  • 1.8 × 1010
  • 85 × 1015
0:0:1


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