TAILIEUCHUNG - Chapter 20: Electrochemistry

Balancing oxidation-reduction equations, oxidation-reduction reactions, voltaic cells, cell EMF, effect of concentration on cell EMF is the main content of the lecture "Chapter 20: Electrochemistry". Invite you to consult the detailed content lectures to capture details. | Copyright 1999, PRENTICE HALL Chapter 20 Electrochemistry Chapter 20 David P. White University of North Carolina, Wilmington 1 1 1 1 Copyright 1999, PRENTICE HALL Chapter 20 Oxidation-Reduction Reactions Zn added to HCl yields the spontaneous reaction Zn(s) + 2H+(aq) Zn2+(aq) + H2(g). The oxidation number of Zn has increased from 0 to 2+. The oxidation number of H has reduced from 1+ to 0. Therefore, Zn is oxidized to Zn2+ while H+ is reduced to H2. H+ causes Zn to be oxidized and is the oxidizing agent. Zn causes H+ to be reduced and is the reducing agent. Note that the reducing agent is oxidized and the oxidizing agent is reduced. Copyright 1999, PRENTICE HALL Chapter 20 Balancing Oxidation-Reduction Equations Law of conservation of mass: the amount of each element present at the beginning of the reaction must be present at the end. Conservation of charge: electrons are not lost in a chemical reaction. In complicated redox reactions, we need to look at the transfer

• Hoá học
• Chapter Electrochemistry
• Standard reduction potentials
• Balancing oxidation
• Reduction equations
• Oxidation reduction reactions
• Voltaic cells
• Lecture General Chemistry 2
• Bài giảng Hóa học đại cương 2
• Chemical electrochemistry
• Electrochemistry work
• Redox reactions
• Balancing redox reactions
• Fundamentals
• Electrochemistry
• Electrodes
• Potentiometry
• Engineering Biotechnology
• Analytical Chemistry
• chemical analysis