Q49.For an electrochemical cell Sn(s) Sn2 + (aq, 1M) Pb2+(aq, 1M) Pb(s) the ratio [Sn2+] when this cell [Pb2+] attains equilibrium is _______ (Given: E0 = −0 .14 V, E0 = −0 .13 V, 2.303RTF = 0 .06 ) Sn2+ Sn Pb2+ Pb
What This Question Tests
The question tests the ability to calculate the standard cell potential, apply the Nernst equation at equilibrium to determine the equilibrium constant, and thus the ratio of ion concentrations.
Concepts Tested
Formulas Used
E°cell = E°cathode - E°anode
Ecell = E°cell - (0.06/n)logQ
Ecell = 0 at equilibrium
Keq = [Products]/[Reactants]
📚 NCERT Sections This Tests
2.4 — Calculate The Standard Cell Potentials Of Galvanic Cell In Which The Following
Chemistry Class 11 · Chapter 2
2.4 Calculate the standard cell potentials of galvanic cell in which the following reactions take place: (i) 2Cr(s) + 3Cd2+(aq) ® 2Cr3+(aq) + 3Cd (ii) Fe2+(aq) + Ag+(aq) ® Fe3+(aq) + Ag(s) Calculate the DrGo and equilibrium constant of the reactions. 2.5 Write the Nernst equation and emf of the following cells at 298 K: (i) Mg(s)|Mg2+(0.001M)||Cu2+(0.0001 M)|Cu(s) (ii) Fe(s)|Fe2+(0.001M)||H+(1M)|H2(g)(1bar)| Pt(s) (iii) Sn(s)|Sn2+(0.050 M)||H+(0.020 M)|H2(g) (1 bar)|Pt(s) (iv) Pt(s)|Br–(0.010 M)|Br2(l )||H+(0.030 M)| H2(g) (1 bar)|Pt(s).
2.2 — Given The Standard Electrode Potentials,
Chemistry Class 11 · Chapter 2
2.2 Given the standard electrode potentials, K+/K = –2.93V, Ag+/Ag = 0.80V, Hg2+/Hg = 0.79V Mg2+/Mg = –2.37 V, Cr3+/Cr = – 0.74V Arrange these metals in their increasing order of reducing power.
2.6 — In The Button Cells Widely Used In Watches And Other Devices The Following
Chemistry Class 11 · Chapter 2
2.6 In the button cells widely used in watches and other devices the following reaction takes place: Zn(s) + Ag2O(s) + H2O(l) ® Zn2+(aq) + 2Ag(s) + 2OH–(aq) Determine DrGo and Eo for the reaction.
📋 Question Details
- Chapter
- Electrochemistry
- Topic
- Nernst equation and Equilibrium Constant
- Year
- 2020
- Shift
- 08 Jan Shift 2
- Q Number
- Q49
- Type
- Numerical
- NCERT Ref
- Class 12 Chemistry Ch 3: Electrochemistry
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