Oxygen overpotential
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This document discusses oxygen overvoltage and overpotential. It explains that oxygen overvoltage is the difference between the theoretical oxygen reduction potential of +1.23 V and the experimentally observed electrode potential. It occurs because oxygen reduction involves multiple steps - the oxidation of water to oxygen gas and protons, and then the reverse reduction of oxygen and protons back to water. These multi-step reactions contribute to an overpotential above the theoretical potential. The document also includes the electrochemical series and diagrams showing how concentration gradients and distance from the electrode surface can contribute to overvoltage.
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This document discusses oxidation-reduction (redox) reactions. It defines oxidation as the loss of electrons and reduction as the gain of electrons. Redox reactions always involve a transfer of electrons between reactants. The key principles are:
1. Oxidation and reduction always occur together in a redox reaction.
2. The total number of electrons lost must equal the total number of electrons gained to satisfy the conservation of charge.
3. Redox titrations can be used to determine the concentration of an unknown substance and rely on a redox reaction between a titrant and analyte with an indicator or potentiometer used to find the endpoint.
Electrochemistry
This document provides an overview of electrochemistry and galvanic cells. Some key points:
- Electron transfer reactions are oxidation-reduction (redox) reactions that can generate electric current or be driven by an applied current, making it the field of electrochemistry.
- Galvanic cells use spontaneous redox reactions to generate electricity, with oxidation occurring at the anode and reduction at the cathode. The potential difference between electrodes is called the cell voltage.
- Standard electrode potentials (E°) describe the tendency of half-reactions to occur and can be used to predict spontaneity of redox reactions in cells. Nernst equation relates cell potential to concentrations.
Redox Reaction
This document discusses oxidation-reduction (redox) reactions. It defines redox reactions as those involving the loss or gain of electrons. The reactant that loses electrons (gets oxidized) is the reducing agent, while the reactant that gains electrons (gets reduced) is the oxidizing agent. Oxidation is defined as the loss of electrons, while reduction is the gain of electrons. The document also provides examples of variable valence elements that can exist in different oxidation states and outlines the steps for balancing redox equations under acidic and basic conditions.
2-Electrochemistry.pptx
The document provides an overview of electrochemistry concepts including:
- Reference electrodes like the standard hydrogen electrode and calomel electrode are used to measure electrode potentials.
- The electrochemical series arranges metals based on their electrode potentials and can predict displacement reactions and reaction spontaneity.
- The Nernst equation relates cell potential to standard potential and activity of products and reactants, allowing prediction of cell potential under non-standard conditions.
- Key applications of concepts like the electrochemical series, equilibrium constants, and Nernst equation include calculating standard cell potentials and determining reaction feasibility and direction.
9-redox-equilibrium.pptx
The document provides information on redox reactions including:
- Defining oxidation and reduction in terms of electron loss and gain.
- Explaining how to deduce the oxidation number of elements in compounds and use oxidation numbers to name compounds.
- Stating that redox reactions involve the transfer of electrons between chemical species.
- Describing how to write half reactions to show electron transfer and combine them to give overall redox equations.
- Explaining how to assign oxidation numbers and use them to determine if an element is oxidized or reduced in a reaction.
Redox titration
Linus Pauling was a chemist who received two unshared Nobel Prizes, one for chemistry and one for peace. He made important contributions to fields like chemical bonding and crystallography. This photo shows Pauling tossing an orange, symbolizing his work determining vitamin C levels in fruits using redox titrations with iodine. Redox titrations allow the concentration of ascorbic acid to be measured at various levels in fruits and supplements. The document then provides background information on oxidation-reduction reactions and redox titrations.
Class 10 l Science l Chemistry l Lesson 1: Chemical equations and reactions
A chemical reaction involves one or more reactants forming new products with different properties. Chemical equations represent reactions symbolically, with balanced equations showing equal numbers of atoms on both sides. There are several types of reactions including combination, decomposition, exothermic/endothermic, displacement, neutralization, and oxidation-reduction. Identification of a reaction can occur through changes in state, color, gas evolution, temperature change, or precipitate formation.
Ch4 Reactions in Aqueous Solution
This document discusses various topics related to aqueous solutions and reactions. It begins by defining key terms like solute, solvent, electrolyte and providing examples. It then covers properties of aqueous solutions such as conductivity. Various acid-base reactions and concepts are explained like Brønsted-Lowry acids and bases, neutralization reactions. Oxidation-reduction reactions and oxidation numbers are also discussed. Finally, the document covers concentration of solutions and calculations involving molarity, dilution and preparation of solutions.
23sec3
An electrolytic cell uses electrical energy to drive non-spontaneous redox reactions by pushing electrons from the anode to the cathode. In electrolytic cells, oxidation occurs at the anode and reduction occurs at the cathode, unlike voltaic cells where the reactions are spontaneous. A common example is the electrolysis of water, where applying a current splits water into hydrogen gas at the cathode and oxygen gas at the anode. Electrolysis can also be used to produce chlorine from molten sodium chloride or to electroplate metals onto objects by reducing metal ions at the cathode.
Ch 12 electrochemistry
This document provides an overview of key concepts in electrochemistry, including:
1) Electrochemical cells use spontaneous redox reactions to produce electrical energy through electron transfer along an external path between electrodes.
2) The standard cell potential (ΔE°cell) and free energy change (ΔG°) quantify a redox reaction's tendency to proceed.
3) Half-cell potentials determine ΔE°cell, with the more positive half having a greater tendency for oxidation.
4) The Nernst equation relates cell potential to non-standard state concentrations.
5) Corrosion occurs via redox at metal surfaces, and can be inhibited or protected against.
Electrochemistry by rawat
This document discusses redox reactions and electrochemistry. It covers topics such as oxidation numbers, galvanic cells, cell notation, standard electrode potentials, and how cell potential relates to Gibbs free energy and equilibrium constants. It also discusses corrosion, batteries, fuel cells, and the differences between voltaic, electrolytic, and fuel cells. Redox reactions allow the interconversion of electrical and chemical energy.
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Oxidation and reduction, Balancing the redox rections
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Class 10 l Science l Chemistry l Lesson 1: Chemical equations and reactions
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- 2. Understanding hydrogen overpotential Electrode H+ (aq) e- ½H2(g) Step 1. Reduction of H+ ions to form H atoms H+ (aq) + e– → H Step 2. Adsorption of H atoms on the cathode surface. Step 3. Combination of adsorbed atoms to give hydrogen molecules 2H H2(g)
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- 4. H2 O(l) ½ O2 (g) + 2H+ (aq) + 2e- ½ O2 (g) + 2H+ (aq) + 2e- H2O(l) Oxidation and reduction oxygen Oxidation Reduction
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