We use cookies to improve your experience and understand how Examtube is used. You can accept analytics cookies or continue with essential cookies only.
Privacy policy6 public questions tagged with this topic.
Δr G° = -n F E°cell , -424600 = -n × 96500 × 1.10 . n = (424600/96500 × 1.10) = (424600/106150) ≈ 4 .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
Δr G° = -n F E°cell = -2 × 96500 × 0.44 = -84920 J/mol = -84.92 kJ/mol .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws
Reaction: Fe(s) + 2Ag⁺(aq) → Fe²⁺(aq) + 2Ag(s) . E°cell = E°cathode - E°anode = 0.80 - (-0.44) = 1.24 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
The cell reaction is Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s) . E°cell = E°cathode - E°anode = 0.34 - (-0.76) = 1.10 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
Δr G° = -n F E°cell = -2 × 96500 × 0.77 = -148610 J/mol = -148.61 kJ/mol .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
E°cell = (0.059/n) log Kc . 0.46 = (0.059/2) log Kc , log Kc = 15.59 , Kc ≈ 3.9 × 10¹⁵ .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry
This page is supported by advertisements. An ad blocker is stopping those ads from loading, so we cannot show the rest of the page yet. Pause the blocker for this site, then continue. We will check again automatically.
You can keep using this site after advertisements are allowed to load.
