Cytochrome c oxidase catalyses the transfer of electrons from ferrocytochrome c to molecular oxygen. The balanced equation is shown below. 4 Cytochrome c(Fe 2") + O2 + 4 H*4 Cytochrome c(Fe ")+2H20 The relevant half reactions are: Cytochrome c(Fe ) +eCytochrome c(Fe 2* ) E, = +0.254V 4 O2 + 2 H* +2 e - H20 E = +0.816V (F = Faraday's constant = 96.485 kJ /V. mol, R= 8.314 J/mol.K) (i) What is the standard free energy change for this reaction? (ii) What is the equilibrium constant (K) for this reaction? ......

Cytochrome c oxidase catalyses the transfer of electrons from ferrocytochrome c to molecular oxygen. The balanced equation is shown below. 4 Cytochrome c(Fe 2") + O2 + 4 H4 Cytochrome c(Fe ")+2H20 The relevant half reactions are: Cytochrome c(Fe ) +eCytochrome c(Fe 2 ) E, = +0.254V 4 O2 + 2 H* +2 e - H20 E = +0.816V (F = Faraday's constant = 96.485 kJ /V. mol, R= 8.314 J/mol.K) (i) What is the standard free energy change for this reaction? (ii) What is the equilibrium constant (K) for this reaction? ......

Human Anatomy & Physiology (11th Edition)

11th Edition

ISBN:9780134580999

Author:Elaine N. Marieb, Katja N. Hoehn

Publisher:Elaine N. Marieb, Katja N. Hoehn

Chapter1: The Human Body: An Orientation

Section: Chapter Questions

Problem 1RQ: The correct sequence of levels forming the structural hierarchy is A. (a) organ, organ system,...

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An iron-sulfur protein in Complex 3 donates an electron to cytochrome c1. The reduction half-reactions and Eº' values are shown below. a) write the balanced equation for the reaction and calculate the standard free energy change. b) How can you account for the fact that this reaction occurs spontaneously in the cell? FeS(ox) + e- ---> FeS(red) Eº' = 0.280 V cyt c1 (Fe3+) + e- ---> cyt c1 (Fe2+) Eº' = 0.215 V
Shown below are reduction potentials for four half-reactions. Which of the coupled reactions is favorable? (Note that for Cytochrome c you must multiply the reduction potential by 2 for each coupled reaction because only one electron is involved) a) 2 Cytochrome c (Fe3+) + H2O ó 2 Cytochrome c (Fe2+) + O2 b) NADH + Succinate- ó NAD+ + Fumarate- c) Fumarate- + H2O ó Succinate- + O2 d) All of the above
The turnover number of the enzyme fumarase that catalyzes the reaction, Fumarate + H20 ===→ L-malate, is 2.5 x 103 S - l and Km = 4.0 X 10- 6 mol/L. Calculate the rate of conversion of fumarate to L-malate if the fumarase concentration is 1.0 x 1 0 - 6 mol/L and the fumarate concentration is 2.04 x 10- 4 mol/L.
Write a balanced equation for the oxidation of ubiquinol by cytochrome c. Calculate ΔG°′ and Δℰ°′ for the reaction.
The decomposition reaction of hydrogen peroxide (H₂O₂) proceeds as follows: 2 H₂0₂ → 2 H₂O + 0₂ 2 This reaction can occur without a catalyst, in the presence of a chemical catalyst (platinum) or of a biological catalyst (catalase). 1- From the values given in the table below, determine the catalytic power of each catalyst (ratio of the catalyzed rate of reaction to the uncatalyzed rate). 2- Which catalyst is the most efficient? Reaction conditions No catalyst Platinum Catalase Ea (kJ.mol¹) at 20 °C 75 49 8
The protein catalase is an enzyme that catalyzes the decomposition of hydrogen peroxide:2 H2O2 (aq) → 2 H2O (l) + O2 (g)and has a Michaelis-Menten constant of 25 × 10-3 mol·dm-3 and a turnover number of 4.0×107s-1.The total enzyme concentration is 0.016×10-6 mol·dm-3 and the initial substrate concentration is4.32×10-6 mol·dm-3 Calculate the maximum reaction rate (????) for this enzyme, and the initial rateof this reaction. Note that catalase has a single active site.
Below are the reduction reactions for oxygen and FAD. ½202 + 2e + 2H+ → H20 E°' = 0.83 V FAD + 2e + 2H* → FADH2 E" = -0.22 V What is the potential (E") for the oxidation of FADH by oxygen? What is the AG®' for the oxidation of FADH, by oxygen? If we assume that the pumping of protons in conjunction with the oxidation of FADH, requires 120 kJ, what percentage of the energy from FADH oxidation is stored in the proton gradient (think about how many protons are pumped when FADH, transfers electrons to oxygen)?
The standard free energy change for the reaction catalyzed by phosphoglucomutase is -7.1 kJ/mol. Calculate the equilibrium constant for the reaction. Calculate AG at 37°C when the concentration of glucose-1-phosphate is 1-mM and the concentration of glucose-6-phosphate is 25-mM. Is the reaction spontaneous under these conditions? HOCH, -20;POCH, H H H H H H ОН Н НО ОН Н H НО ОН H ОН H. ОН Glucose-l-phosphate Glucose-6-phosphate
Consider the fructose-1,6-bisphosphatase reaction. Calculate the free energy change if the ratio of the concentrations of the products to the concentrations of the reactants is 23.7, and the temperature is 37.0 °C? AG" for the reaction is -16.7 kJ/mol. The constant R = 8.3145 J/(mol-K) AG= Number kJ/mol
Ozone in the lower atmosphere is a pollutant that can form by the following reaction involving the oxidation of unburned hydrocarbons:CH4(g) + 8 O2(g)-------->CO2(g) + 2 H2O(g) + 4 O3(g)Use the standard free energies of formation to determine ΔG°rxn for this reaction at 25 °C.
For the following reaction[FAD] + 2 cyt c (Fe 2+) + 2 H+ —> [FADH2] + 2 cyt c (Fe+3)determine which of the redox couples is the electron acceptor and which is the electron donor under standard-state conditions, calculatethe value of ΔE and determine the free energy change for the reaction.
Certain bacteria can respire in anoxic environments using arsenic (V) as electron acceptor. The relevant unbalance half reactions are: H₂ AsO+H → H¸AsO +H₂O, logK = 10.84, AG = -14.5kca I m I ol-e CH₂O+H₂OH + CO2 (g), logK = 1.2, AG° = -1.63kca — ol-e 1) Balance the two half reactions 2) What is m the overall respiration reaction, standard free energy change \Delta GO 3) Is this process energetically more or less favorable than sulfate reduction? (\Delta GO for the reduction of sulfate to HS- is -5.78 kcal/mol - e-) 4) If [H2AsO4-] = [ H3ASO3] = 0.5 mM and pH = 7, estimate pe of the system