In Mitochondria Exergonic Redox Reactions

Oxidation-Reduction Reaction of Mitochondria

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The tendency of acids and bases to do­nate or accept protons was described. In acid-base systems, one compound acts every bit the proton (H⁺) donor and the other as the proton acceptor, the donor being the acid and the acceptor the base.

The two form a cohabit acid-base pair. In a like fashion, oxidiz­ing and reducing agents office in pairs.

In this case, they are called redox pairs or redox couples. The member of the pair that donates the electron is chosen the reducing agent or reductant and the electron air conditioning­ceptor is chosen the oxidizing agent or oxidant.

The terms donating and accepting fail to convey the nature of the amounts or energy change involved in the reac­tion. In consequence, the reducing agent has a certain capa­bility to retain electrons, as does the oxidizing agent. In a redox couple, one member attracts electrons more than strongly than the other, and in effect the oxidiz­ing amanuensis can pull the electrons away from the reduc­ing agent. This capability to gain (or lose) electrons tin be measured and is chosen the oxidation- reduction potential or redox potential and is ex­pressed in volts.

For convenience, the potential of almost redox cou­ples is measured confronting a reference standard, which usually is a hydrogen electrode. Most measurements are made under standard conditions using 1.0 Thousand con­centrations of oxidant and reductant at 25 °C and at pH 7.0. The hydrogen electrode is equilibrated with H₂ gas at ane temper and the [H⁺] is 1.0 M at 25°C.

When the pH is adapted to 7.0 (i.eastward., [H⁺] = 10^-7 M), the redox potential of the reference hydrogen electrode is – 0.42 5. The redox potentials of the electron trans­port organization intermediates are given in Tabular array 16-2. The greater the E'_Q value, the more strongly the oxi­dant accepts electrons. However, an oxidant having a lower Eq than another compound becomes the reduc­tant of or electron donor to that chemical compound.

The Henderson-Hasselbach equation  describes the relationship between pH and the dissociation constant. In a similar way, the Nernst equation shows for a redox pair the relationship between the standard redox potential (Eq), the observed potential at whatsoever concentration, and the concentration ratio of the oxidant and reductant.

Where Due east₀' is the standard redox potential, Eastward_h is the ob­served electrode potential, R is the gas abiding (viii.31 J/deg/mole, T is the accented temperature in degrees Kelvin, n is the number of electrons transferred, and F is the faraday (96,406 kJ/V). When electrons are transferred and the constants are combined, the Nernst equation becomes

Where n = the number of electrons involved.

In Mitochondria Exergonic Redox Reactions,

Source: https://www.biologydiscussion.com/mitochondria/oxidation-reduction-reaction-of-mitochondria/3899

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