'Standard reduction potentials' presentation slideshows

Electrochemistry

Electrochemistry. Chapter 17. Contents. Galvanic cells Standard reduction potentials Cell potential, electrical work, and free energy Dependence of cell potential on concentration Batteries Corrosion Electrolysis Commercial electrolytic processes. 17.1 Galvanic Cells.

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Chapter 6 Biological Oxidation

Chapter 6 Biological Oxidation. The biochemistry and molecular biology department of CMU. Biological oxidation is the process in which substances (carbohydrate, Lipid, AAs) are oxidized in living organism. Oxidation types: Dehydrogenation Electron lost Oxygenation.

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Chapter 20 - Electron Transfer Reactions

Chapter 20 - Electron Transfer Reactions. Objectives: 1. Carry out balancing of redox reactions in acidic or basic solutions; 2. Recall the parts of a basic and commercial voltaic cells; 3. Perform cell potential calculations from standard reduction potentials;

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Electrochemistry

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Chapter 19 OXIDATIVE PHOSPHORYLATION AND PHOTOPHOSPHORYLATION

Lehninger Principles of Biochemistry, Fourth Edition, 2005. Chapter 19 OXIDATIVE PHOSPHORYLATION AND PHOTOPHOSPHORYLATION. ????? ??????? ??? ?? June 12, 2007 . 19.1 Electron-Transfer Reactions in Mitochondria. Electrons Are Funneled to Universal Electron Acceptors

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Electrochemistry

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Electrochemistry

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ELECTROCHEMISTRY Chapter 21

ELECTROCHEMISTRY Chapter 21. redox reactions electrochemical cells electrode processes construction notation cell potential and ?G o standard reduction potentials (E o ) non-equilibrium conditions (Q) batteries corrosion. Electric automobile. - 2 e-. 2 x +1 e-.

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ELECTROCHEMISTRY Chapter 21

ELECTROCHEMISTRY Chapter 21. redox reactions electrochemical cells electrode processes construction notation cell potential and ?G o standard reduction potentials (E o ) non-equilibrium conditions (Q) batteries corrosion. Electric automobile.

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Redox Reactions in Metabolism: Standard reduction potentials, coenzymes in metabolism, and pyruvate dehydrogenase

Redox Reactions in Metabolism: Standard reduction potentials, coenzymes in metabolism, and pyruvate dehydrogenase. Bioc 460 Spring 2008 - Lecture 27 (Miesfeld). NADH. Acetyl-CoA. Vitamins are organic compounds in nature that were discovered through dietary deficiency diseases such as beriberi.

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Topic 12 Electrochemistry

Topic 12 Electrochemistry. Review. Oxidation reduction reactions involve a transfer of electrons. OIL- RIG Oxidation Involves Loss Reduction Involves Gain LEO-GER Lose Electrons Oxidation Gain Electrons Reduction. Applications. Moving electrons is electric current.

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Oxidation and Reduction

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Oxidation and Reduction

Oxidation and Reduction. as it pertains to biochemistry. please read . Read The Slow Burn. fig 13-22. fig 13-22. reduction potential can be measured. ref. cell. test cell. fig 13-23. Redox reactions as pairs of half-reactions. Fe 3+ + Cu +. Fe 2+ + Cu 2+.

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Electrochemistry

Electrochemistry. Redox reactions. The half-reactions for Sn 2+ ( aq ) + 2Fe 3+ ( aq ) ? Sn 4+ ( aq ) + 2Fe 2+ ( aq ) are Oxidation: Sn 2+ ( aq ) ? Sn 4+ ( aq ) +2e- Reduction: 2Fe 3+ ( aq ) + 2e- ? 2Fe 2+ ( aq ) In oxidation: electrons are products.

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Lecture 12: Cell Potentials

Lecture 12: Cell Potentials. Reading: Zumdahl 11.2 Outline What is a cell potential? SHE, the electrochemical zero. Using standard reduction potentials. Cell Potentials.

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Electrochemistry

Electrochemistry. Redox reactions. electrochemical cells galvanic : spontaneous chemical rxns to produce electrical energy ( D G = -nFE, negative) electrolytic : utilisation of energy (ex: applied V) to force a chemical rxn to take place ( D G +). Cells.

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Galvanic (or Voltaic) Cells

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The oxidation states of vanadium

The oxidation states of vanadium. Objectives: access multiple oxidation states of V separate compounds via ion exchange chromatography. Vanadium Complexes in This Lab. [V(H 2 O)] 6 2+ [V(H 2 O) 6 ] 3+ [V(H 2 O) 5 O] 2+ [V(OH)O 3 ] 2- Draw 3D structure Give oxidation number of V.

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Classification of Chemical Reactions

Classification of Chemical Reactions. Notes. Composition (also called combination or synthesis). Two reactants combine to form one product A + B ? AB Example: 3Na + P ? Na 3 P Helpful hints

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