Q59.Consider the cell at 25°C ZnZn2 + aq, 1 M‖Fe3 + (aq), Fe2 + aqPts The fraction of total iron present as Fe3 + ion at the cell potential of 1 . 500 V is x × 10-2. The value of x is ______. (Nearest integer) Given: E∘ + + = 0 . 77V, E∘ + = - 0 . 76V Fe3 | Fe2 Zn2 | Zn
What This Question Tests
This question requires applying the Nernst equation to calculate the concentration ratio of Fe3+ to Fe2+ ions in a galvanic cell at a given cell potential.
Concepts Tested
Formulas Used
Ecell = E°cell - (0.0592/n) logQ
E°cell = E°cathode - E°anode
📚 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).
2.9 — The Resistance Of A Conductivity Cell Containing 0.001M Kcl Solution At 298
Chemistry Class 11 · Chapter 2
2.9 The resistance of a conductivity cell containing 0.001M KCl solution at 298 K is 1500 W. What is the cell constant if conductivity of 0.001M KCl solution at 298 K is 0.146 × 10–3 S cm–1. 59 Electrochemistry Reprint 2025-26
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
- Year
- 2021
- Shift
- 25 Jul Shift 1
- Q Number
- Q59
- Type
- Numerical
- NCERT Ref
- Class 12 Chemistry Ch 3: Electrochemistry
More from this Chapter
Q58.The mass of product liberated on anode in an electrochemical cell depends on (where t is the time period, for which the current is passed) (1) (It)1/2 (2) IT (3) I/t (4) I2t
Q48.The negative Zn pole of a Daniell cell, sending a constant current through a circuit, decreases in mass by 0.13 g in 30 minutes. If the electrochemical equivalent of Zn and Cu are 32.5 and 31.5 respectively, the increase in the mass of the positive Cu pole in this time is (1) 0.180 g (2) 0.141 g (3) 0.126 g (4) 0.242 g
Q49.The electrochemical equivalent of a metal is 3.3 × 10−7 kg per coulomb. The mass of the metal liberated at the cathode when a 3 A current is passed for 2 seconds will be (1) 19.8 × 10−7 kg (2) 9.9 × 10−7 kg (3) 6.6 × 10−7 kg (4) 1.1 × 10−7 kg
Q46.Two voltameters one of copper and another of silver, are joined in parallel. When a total charge q flows through the voltameters, equal amount of metals are deposited. If the electrochemical equivalents of copper and silver are z1 and z2 respectively the charge which flows through the silver voltameter is (1) q z1 (2) q z2 1+ 1+ z2 z1 (3) q z1 (4) q z2 z2 z1