### Mitochondrial Electron Transport Adaptation2. **Unique Electron Acceptor in Mitochondrial Electron Transport**: - **Observation**: A cell is discovered to use Cu²⁺ as the final electron acceptor in mitochondrial electron transport (MET) instead of O₂. - **Reaction**: \[ \text{Cu}^{2+} + 2e^- \leftrightarrow \text{Cu}^0 \] \[ \text{E}^\circ = +0.337 \, \text{V} \] - **Problem Statement**: **A. Calculation of Free Energy**: Determine how much free energy can be gained by the oxidation of NADH in this novel MET system. Show calculations.### Detailed ExplanationThe reduction potential (Eº) for the half-reaction provided is +0.337 V for Cu²⁺/Cu⁰. To determine the free energy change (ΔG) from the oxidation of NADH, we need to use the Nernst equation and the known standard reduction potential for NADH/NAD⁺.Key Steps for Calculation:1. **Identify the standard reduction potentials**: - For Cu²⁺ + 2e⁻ → Cu⁰: Eº = +0.337 V - For NAD⁺ + H⁺ + 2e⁻ → NADH: Eº = -0.320 V2. **Calculate the overall cell potential (Eºcell)**: \[ \text{Eº} = \text{Eº (electron acceptor) - Eº (electron donor)} \] \[ \text{Eºcell} = 0.337 \, \text{V} - (-0.320 \, \text{V}) = 0.657 \, \text{V} \]3. **Use the Gibbs free energy equation**: \[ \Delta G = -nFEºcell \] where: - \( n \) = number of moles of electrons exchanged (n = 2 for NADH oxidation reaction) - \( F \) = Faraday constant (approximately 96485 C/mol) - \( Eºcell \) = total cell potential (0.657 V)4. **

Given : We have to calculate free energy .

You discover a cell that uses Cu² as the final electron acceptor in mitochondrial electron transpo (MET) instead of O. Cu* + 2e e → Cu° E°=+0.337 V A. How much free energy can be gained by oxidation of NADH in this novel MET system? Show calculations.

You discover a cell that uses Cu² as the final electron acceptor in mitochondrial electron transpo (MET) instead of O. Cu* + 2e e → Cu° E°=+0.337 V A. How much free energy can be gained by oxidation of NADH in this novel MET system? Show calculations.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Identify the strongest reducing agent from the given reaction: Choose among a.H2O2 b.NADH c.NAD+ d.O2 Given reaction: oxaloacetate + 2H+ +2e- ↔ malate Eo=+0.330 V NAD+ + H+ + 2 e- ↔ NADH Eo = - 0.105 V O2(g) + 2H+ + 2e- ↔ H2O2 Eo = +0.695 V
3. Tanjiro, a Chem 17.1 student, found a prehistoric katana during his trip to Japan. He inspected the katana and realized that it was made out of gold. Upon closer inspection, Tanjiro noticed that it had a lot of chips and scratches, signifying that it had been used in battle long ago. Wanting to restore the katana to its original state, Tanjiro used his knowledge in Chem 17.1 to electroplate gold into the surface of the katana using an ore his father found on their backyard. Tanjiro proceeded with the electroplating process, however, he realized that the concentration of the gold ions present in the solution is unknown, making the electroplating process difficult to plan. He then decided to use a galvanic cell to obtain the gold ion concentration. He used the half-cell reactions below: Au³+ (aq) + 3e → Au(s) E° = +1.520V E° = -0.230V Ni²+ (aq) + 2e → Ni(s) Given: [Ni²+] = 0.050 M FMNI = 58.69 g/mol FMAU = 196.97 g/mol
Which statements is/are true? a. At the start of the electrochemical reaction, the cell potential (Ecell) of a concentration cell is always zero. b. If 25 mmol of Gd metal forms after electrolysis of Gd ions using a current of 1.0 A for 2 h, the Gd source has a charge of +3.
Which of the following is true for the cell below? Zn(s) | Zn2+(aq) ‖ Cr3+ (aq) | Cr(s) * The cations flow from the cathode to the anode. * The electrons flow from the anode to the cathode. * The chromium is oxidized. * The anions flow from the anode to the cathode. * The zinc is reduced.
None
12.
Show your work please, thank you!
Calculate the pK for the oxidation of X by Hplus at 25 degrees C. X(s) + 3 Hplus → X3 plus (aq)+ 3/2 H2(g) The reduction potential of X3 plus is 0.42 V. Report your answer with two decimal places.
consider the following standard reduction potentials
Write the line notation for the following cell. Pt HBr(aq, 0.10 M) Line notation: Br₂(/) AI(NO3)3(aq, 0.010 M) Al AI(NO3)3(aq, 0.010 M) Answer Bank HBr(aq, 0.10 M) Pt(s) Al(s) Br₂ (1)
Calculate the standard potential, ?∘, for this reaction from its Δ?∘ value. X(s)+Y2+(aq)⟶X2+(aq)+Y(s)Δ?∘=−16.0 kJ
For the cell at 298 K outlined below, answer the questions. The cell volumes are 100.0 ml. Au (s) | Au3+ (0.8 M) || Ag+ (0.6 M) | Ag (s) What is DeltaG of the cell? If a current of 1.2 amps is drawn from the cell for 10800 seconds. What is Ecell at that point?