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ChemistryNEET 2019Electrochemical cells and Nernst equation

Electrochemistry

For the cell reaction 2Fe3+(aq)+2I−(aq)→2Fe2+(aq)+I2(aq)2\mathrm{Fe^{3+}(aq) + 2I^-(aq) \to 2Fe^{2+}(aq) + I_2(aq)}, Ecell⊖=0.24E^\ominus_{cell} = 0.24 V at 298 K. The standard Gibbs energy (ΔrG⊖\Delta_r G^\ominus) of the cell reaction is: (Given: Faraday constant F=96500 C mol−1F = 96500\ \mathrm{C\,mol^{-1}})

  1. A.−46.32 kJ mol−1-46.32\ \mathrm{kJ\,mol^{-1}}✓
  2. B.−23.16 kJ mol−1-23.16\ \mathrm{kJ\,mol^{-1}}
  3. C.46.32 kJ mol−146.32\ \mathrm{kJ\,mol^{-1}}
  4. D.23.16 kJ mol−123.16\ \mathrm{kJ\,mol^{-1}}

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