Question

The cytochromes are heme‑containing proteins that function as electron carriers in the mitochondria. Calculate the difference in the reduction potential (ΔE∘′) and the change in the standard free energy (ΔG∘′) when the electron flow is from the carrier with the lower reduction potential to the higher. cytochrome c1 (Fe3+)+e−↽−−⇀cytochrome c1 (Fe2+)E∘′=0.22 V cytochrome c (Fe3+)+e−↽−−⇀cytochrome c (Fe2+)E∘′=0.254 V Calculate ΔE∘′ and ΔG∘′ .

Answer 1

Complete Question

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Answer:

The change in reduction potential is  $\Delta E^o=E^o_{cell} = 0.034 V$

The change in standard free energy is  $\Delta G^o = -3.2805 \ KJ/mol$

Explanation:

From the question we are told that

At the anode

      $cytochrome \ c_1 \ (Fe^{3+}) + e^-$⇔$cytochrome \ c_1 \ (Fe^{2+}) \ \ E^o = 0.22 \ V$

At the cathode

      $cytochrome \ c \ (Fe^{3+}) + e^-$⇔$cytochrome \ c \ (Fe^{2+}) \ \ E^o = 0.254 \ V$

The difference in the reduction potential is mathematically represented as

     $\Delta E^o = E^o_{cathode} - E^o_{anode}$

substituting values

      $\Delta E^o = 0.254 - 0.220$

     $\Delta E^o=E^o_{cell} = 0.034 V$

The change in the standard free energy is mathematically represented as

      $\Delta G^o = -n * F * E^o_{cell}$

Where  F is the Faraday constant with value  F = 96485 C

and  n i the number of the number of electron = 1

   So

       $\Delta G^o = -(1) * 96485 * 0.034$

       $\Delta G^o = -3.2805 \ KJ/mol$