redoxtherm
TRANSCRIPT
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Oxidation-Reduction
important reaction type in biochemistry
Electron transfer reaction
many different types of reactions
Oxidation and reduction have to occur simultaneously
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Definitions
Reduction
Gaining of electrons
Loss of oxygen
Gaining of Hydrogen
Oxidation
Loss of electrons
Gaining of oxygen
Loss of Hydrogen
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Loss of electrons/Gaining of electrons
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Loss of electrons/Gaining of electrons
• Which species is being oxidized?• Which species is being reduced?• Importance of this reaction? • One step in gluconeogenesis (formation of
glucose)• The reverse reaction occurs when vigorously
contracting muscles function under low oxygen conditions
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Thermodynamics
• Study of energy• Important to understanding biochemistry• Two key terms:
• Enthalpy H : Heat of reaction at constant pressure
• Endothermic: Require heat +H
• Exothermic: Releases heat -H
• Change in Entropy S : Change in Randomness
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First Law of Thermodynamics
• Energy is conserved during the course of a chemical change
• Energy can be transformed into one form from another
• Energies: Potential, Kinetic, Light, Heat• Example: What happens when you dive off a
diving board into a pool?
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Second Law of Thermodynamics
S univ> 0 for a Spontaneous Reaction
• What does this mean?
• Reactions happen without outside intervention when the entropy (randomness) of the universe increases. S univ is the change in entropy
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Spontaneous Reactions
• Spontaneous Reactions are Thermodynamically Favored Reactions
• Entropy of the universe (S univ)=entropy of the system + entropy of surroundings
• The change in entropy of univ has to be positive S univ> 0 for a spontaneous reaction. • Note that S system can be negative if Ssurroundings is
sufficiently positive to overcome it • Examples:
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Spontaneous Reactions
• Gibbs-Helmhotz equation describes the second law in terms of Free energy (G)
• Free energy is derived from the Second Law. It is the same thing using different terms.
• It is the amount of work that the system can do or the amount of work needed for the system
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•Spontaneous Reactions
• Free energy has to be released from the system if the process is spontaneous
• For a spontaneous process: Gsys is negative or Gsys < 0• These reactions are thermodynamically favored• These reactions are said to be exergonic• Amount of energy available to do work
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Non-Spontaneous Process
• For a non-spontaneous process: S univ < 0
Gsys is positive or Gsys > 0• These reactions are not thermodynamically
favored• These reactions are said to be endergonic
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Exergonic vs. Endergonic Reactions
• Products have more energy than reactants
• Energy gained by system
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Exergonic v. endergonic reactions
• Products have less energy than reactants
• Energy released• Available to do work• spontaneous
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Linking of exergonic to endergonic reactions (reaction coupling)
• In biochemical systems, an exergonic reaction is used to drive an endergonic one
• In other words, the free energy released in one reaction is used as the free energy needed in another reaction
• Example: cooking food• Example: Hydrolysis of ATP is used in many
reactions to drive another reaction such as formation of macromolecules
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The Big Picture Energy Interconversion in Living Organisms
What is the relationship between energy, metabolism, heat, and
entropy?
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The Big Picture Energy Interconversion in Living Organisms
• There is Potential Energy Stored in Nutrients (animal cell) or Sunlight (plant cell)
• Convert some of this potential energy through chemical transformations in the cell to do work
• Macromolecules within the cell are formed: Entropy is decreased in the system
• However, products of metabolism (CO2 for example) increase the randomness of the surroundings
• Heat is given off increasing the randomness of the surroundings
• Overall, S univ >0
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