The standard Gibbs energy for the given cell reaction in kJ mol^–1 at 298 K is: Zn(s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu (s), E° = 2 V at 298 K (Faraday's constant, F = 96000 C mol^–1)

Redox Reactions and Electrochemistry: JEE Main 2019 Chemistry question

JEE Main 2019 · 9 Apr, Morning shift · Q987

JEE Main 20199 Apr, Morning shiftChemistryEasyRedox Reactions and Electrochemistry138× since 2002

The standard Gibbs energy for the given cell reaction in kJ mol^–1 at 298 K is : Zn(s) + Cu²⁺ (aq)

\to

Zn²⁺ (aq) + Cu (s), E° = 2 V at 298 K (Faraday's constant, F = 96000 C mol^–1)

JEE Main 2019 · 9 Apr, Morning shift · Q987

JEE Main 20199 Apr, Morning shiftChemistryEasyRedox Reactions and Electrochemistry138× since 2002

The standard Gibbs energy for the given cell reaction in kJ mol^–1 at 298 K is : Zn(s) + Cu²⁺ (aq)

\to

Zn²⁺ (aq) + Cu (s), E° = 2 V at 298 K (Faraday's constant, F = 96000 C mol^–1)