Q49.The reduction potential of hydrogen half cell will be negative if : (1) p (H2) = 1 atm and [H+] = 1.0M (2) p (H2) = 2 atm and [H+] = 1.0M (3) p (H2) = 2 atm and [H+] = 2.0M (4) p (H2) = 1 atm and [H+] = 2.0M
What This Question Tests
This question requires applying the Nernst equation to the hydrogen half-cell to determine the conditions under which its reduction potential becomes negative, testing conceptual understanding of electrode potentials.
Concepts Tested
Formulas Used
E_reduction = E°_reduction - (0.0591/n) * log(P(H2) / [H+]²)
📚 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.
2.9 — 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
📋 Question Details
- Chapter
- Electrochemistry
- Topic
- Nernst Equation for Standard Hydrogen Electrode (SHE)
- Year
- 2011
- Shift
- Unknown
- Q Number
- Q49
- Type
- MCQ
- NCERT Ref
- Class 12 Chemistry Ch 3: Electrochemistry
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