JEE Questions for Chemistry Electrochemistry Quiz 5 - MCQExams.com


Chemistry-Electrochemistry-3295.png
  • Weston cell
  • Daniell cell
  • Calomel cell
  • Faraday cell
Aluminium displaces hydrogen from acids but copper does not. A galvanic cell prepared by combining Cu / Cu2+ and Al/ Al3+ has an emf of 2.0 V at 298 K. If the potential of copper electrode is +0.34 V, that of aluminimum electrode is
  • - 2.3 V
  • + 2. 34 V
  • -1.66 V
  • + 1.66 V
The standard emf. of a cell Zn/Zn2+|| Fe2+/Fe, if electrode potentials for (Zn/Zn2+) and (Fe2+/Fe) are 0.763 V and - 0.44 V respectively is
  • + 0.323 V
  • - 1.203 V
  • + 1.203 V
  • - 0.323 V
The electrochemical cell shown below is a concentration cell. M / M2+ (saturated solution of a sparingly soluble salt, MX2) 11M2+ (0.00001 mol dm-3/ M) . The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298 is 0.059 V. The value of ∆G (kJ mol-1 ) for the given cell is (take 1F = 96500C mol-1 )
  • - 5.7
  • 5.7
  • 11.4
  • - 11.4
In which of the following case, increase in concentration of ion cause increase in Ecell?
  • Pt(H2)|H+ (aq)
  • Pt|Quinhydrogen| H+ (aq)
  • Ag|Ag+ (aq)
  • Ag, AgCl|Cl- (aq)
Out of Cu, Ag Fe and Zn, the metal which can displace all others from their salt solution is
  • Zn
  • Cu
  • Ag
  • Fe

Chemistry-Electrochemistry-3297.png
  • 2 × 102
  • 3 × 102
  • 2 × 105
  • 10
Which one of the following has a potential more than zero?
  • Pt, 1/2 H2 (1 atm)| HCl (2M)
  • Pt, 1/2 H2 (1 atm)| HCl (0.1M)
  • Pt, 1/2 H2 (1 atm)| HCl (0.5M)
  • Pt, 1/2 H2 (1 atm)| HCl (1M)

Chemistry-Electrochemistry-3300.png
  • Mg, Ag, Cu
  • Mg, Cu, Ag
  • Ag, Hg, Cu
  • Cu, Hg, Ag
Consider the following cell reaction
2 Fe (s) + O2 (g) + 4H+ (aq) →2Fe2+ (aq) + 2H2O(l), Eo = 1.67 V
At [Fe2+] = 10-3 M, po2 = 0.1 atm and pH = 3, the cell potential at 25oC is
  • 1.47 V
  • 1.77 V
  • 1.87 V
  • 1.57 V
The reduction potential of hydrogen half-cell will negative if
  • p(H= 1 atm and [H+] = 2.0M
  • p(H= 1 atm and [H+] = 1.0M
  • p(H= 2 atm and [H+] = 1.0M
  • p(H= 2 atm and [H+] = 2.0M
E1, E2, E3 are the emfs of the following three galvanic cells respectively
I. Zn (s) | Zn2+ (0.1M) ||Cu2+ (1 M)|Cu (s)
II. Zn (s) |Zn2+ (1M)||C2+ (1M)|Cu (s)
III. Zn(s) |Zn2+ (1M)|| Cu2+ (0.1M)|Cu (s)
Which one of the following is true ?
  • E2 > E1 > E3
  • E1 > E2 > E3
  • E3 > E1 > E2
  • E3 > E2 > E1
The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the redox reaction of the cell is
  • 1020
  • 105
  • 10
  • 1010
The standard redox potentials for the reactions
Mn2+ + 2e- → Mn and Mn3+ + e- → M2+
are - 1.18 V and 1.51 V respectively . What is the redox potential for the reaction Mn3+ + 3e- → Mn ?
  • 0.33 V
  • 1.69 V
  • -0.28 V
  • -0.85 V
  • 0.85 V
The standard reduction potential Eo for half reactions are
Zn = Zn+ + Ze, Eo = + 0.76 V
Fe = Fe2+ + Ze, Eo = + 0.41 V
The emf of the cell reaction
Fe2+ + Zn = Zn2+ + Fe is
  • - 0.35 V
  • +0.35 V
  • +1.17 V
  • - 1.17 V
Which of the following reactions is correct for a given electrochemical cell at 25°C?
Pt | Br2(g) | Br- (g) || Cl- (aq) | Cl2(g) | Pt
  • 2Br- (aq) + Cl2 (g) → 2Cl- (aq) + Br2 (g)
  • Br2 (g) + 2Cl- (aq) → 2 Br- (aq) + Cl2 (g)
  • Br2 (g) + Cl2(g) → 2Br- (aq) + 2Cl- (aq)
  • 2Br- (aq) + 2Cl- (aq) → Br2 (g) + Cl2 (g)
What will be the electrode potential of that hydrogen electrode is filled with HCl solution of pH value 1.0?
  • - 59.15 V
  • + 59.15 V
  • + 59.15 mV
  • - 59.15 mV

Chemistry-Electrochemistry-3305.png
  • II
  • I
  • III
  • All of these
At 25oC temperature the cell potential of a given electrochemical cell is 1.92 V. Find the value of x.
Mg (s) | Mg2+ (aq) x M ||Fe2+ (aq) 0.01M| Fe (s)
Eo Mg / Mg2+ (aq) = 2.37 V; Eo Fe/ Fe2+ (aq) = 0.45 V
  • x = 0.01 M
  • x < 0.01 M
  • x > 0.01 M
  • x cannot be predicted
The emf of the cell Ni|Ni2+ (1.0M)|| Au3+ (1.0M)| Au is [Eo(Ni2+/Ni) = -0.25 V and Eo (Au3+/Au) = + 1.5V]
  • 2.00 V
  • 1.25 V
  • - 1.25 V
  • 1.75 V

Chemistry-Electrochemistry-3306.png
  • -0.072 V
  • 0.385 V
  • 0.770 V
  • -0.270 V
Daniel cell, anode and cathode are, respectively
  • Zn|Zn2+ and Cu2+| Cu
  • Cu|Cu2+ and Zn2+| Zn
  • Fe|Fe2+ and Cu2+|Cu
  • Cu|Cu2+ and Fe2+|Fe
The potential of the following cell is 0.34V at 25°C. Calculate the standard reduction potential of the copper half-cell.
Pt | H2 (1 atm) | H+ (1 M) || Cu2+ (1 M) | Cu
  • -3.4 V
  • +3.4 V
  • -0.34 V
  • + 0.34 V
The potential of the cell for the reaction,
M (s) + 2 H+ (1M) → H2 (g) (1 atm) + M2+ (0.1M) is 1.500 V. The standard reduction potential for M2+/ M (s) couple is
  • 0.1470 V
  • 1.470 V
  • 14.70 V
  • None of these
Small quantities of solutions of compounds TX , TY and TZ are put into separate test tubes containing X ,Y and Z solutions. TX does not react with any of these. TY reacts with both X and Z. TZ reacts with X. The decreasing order of ease of oxidation of the anions X-, Y-, Z- is
  • Y-, Z-, X-
  • Z-, X-, Y-
  • Y-, X-, Z-
  • X-, Z-, Y-

Chemistry-Electrochemistry-3309.png
  • 0.26 V
  • 0.399 V
  • -0.339 V
  • -0.26 V
The standard reduction potentials at 298 K for the following half-cell reactions are given
Zn2+ (aq) + 2e- ⇌ Zn(s); -0.762 V
Cr3+ (aq) + 3e- ⇌ Cr(s); -0.74 V
2H+ (aq) + 2e- ⇌ H2 (g); +0.00 V
Fe3+ (aq) + e- ⇌ Fe2+ (aq); +0.77 V
Which one of the following is the strongest reducing agent ?
  • Zn(s)
  • Cr(s)
  • H2(s)
  • Fe2+ (aq)
Electrode potential of hydrogen electrode is...volt.
  • 0
  • +1
  • -1
  • None of these
The relationship between Gibbs' free energy change (∆G) and emf(E)of a reversible electrochemical cell is given by
  • ∆G = nFE
  • ∆G = nF/E
  • ∆G = - nFE
  • ∆G = E/nF
Zn2+ → Zn(s); Eo = -0.76 V;
Cu2+ → Cu(s); Eo = -0.34 V
Which of the following is spontaneous?
  • Zn2+ + Cu → Zn + Cu2+
  • Cu2+ + Zn → Cu + Zn2+
  • Zn2+ + Cu2+ → Zn + Cu
  • None of these
0:0:1


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