Electrochemistry Review - Cell Potential & Notation, Redox Half Reactions, Nernst Equation
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- Опубліковано 19 чер 2016
- This electrochemistry review video tutorial provides a lot of notes, equations, and formulas that you need to pass your next chemistry test / exam. It’s a nice video that provides an introduction or overview of electrochemistry including the most important fundamental topics and concepts. It contains plenty of examples and practice problems.
Intro to Galvanic & Voltaic Cells:
• Introduction to Galvan...
How To Draw Galvanic Cells:
• How To Draw Galvanic C...
Standard Reduction Potentials:
• Standard Reduction Pot...
Cell Potential Problems:
• Cell Potential Problem...
Cell Notation Problems:
• Cell Notation Practice...
___________________________________
Concentration Cells:
• Concentration Cells & ...
Cell Potential & Gibbs Free Energy:
• Cell Potential & Gibbs...
Cell Potential & Equilibrium K:
• Equilibrium Constant K...
Nernst Equation:
• Nernst Equation Explai...
Electrolysis of Water:
• Electrolysis of Water ...
_____________________________________
Electrolysis of Sodium Chloride:
• Electrolysis of Sodium...
Electrolysis & Electroplating Problems:
• Electrolysis & Electro...
Electrochemistry Practice Problems:
• Electrochemistry Pract...
SAT Chemistry Subject Test Review:
• SAT Chemistry Subject ...
Carbon -14 Dating:
• Carbon 14 Dating Probl...
Beer Lambert's Law:
• Beer Lambert's Law, Ab...
______________________________________
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At 34.26 minutes of video,
∆G = ∆G^o - RT lnQ
I have 2 textbook here of Gen Chemistry saying that
∆G = ∆G^o + RT lnQ
^o is to superscript, to set delta G in standard state
I am learning a lot from you but I like to clarify this formula..Thank you.
The textbooks are:
Fundamentals of Chemistry, 4th Ed. by Frank Brescia etc. page 311
Principles of General Chemistry, 3rd edition by Martin S. Silberberg, page 676
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At 58:26, If you multiply the reaction by 2, wouldn't the half reaction then be 1.54V? And the new total would be 1.77V?
edit: 1:03:12 The answer is no.
If the reaction is multiplied by a coefficient the cell potential won't be affected or altered.
It is only altered when the reaction is reversed.
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How does he know, the concentration for Zn^2+ and Cu^2+. That it is 0,01 and 10?? Please answer
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2:16 What if We plug in the battery to outlet and to my device at the same time..... it's (the battery) is receiving energy (electrolytic) and also supplying energy (galvanic).....how does this work ?
How is zinc the product and copper is the reactant if the copper is gaining mass in the cell?
Mark Keith, this reaction is not about product or reactant. It's electro chemical reaction pertaining to cell. We call them product/reactant only to simplify.
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whilst most of the content was fairly clear, i was a little mystified at the end where predictions were made as to reaction products at anode and cathode. In my hands on experience, if using HCL as the electrolyte/solvent, you normally see Cl2 being generated at the anode and a codeposition of H2 gas and copper on the cathode. If using H2SO4 as electrolyte, water will be oxidised to O2 at the anode and you still see H2 gas and Cu deposition at the cathode.
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In which part of the video can I find half cell equations involving ions and gases
58:14 it is 1 volt
yes I also got 1.0 V
On the last question what happened to "the one with the most positive cell potential will run as reduction" why was there are exception for cl2
can you discuss regarding how Electro Chemistry apply in waste water treatment and Metal recover from Electronic Industry waste water with Copper and or lead particles in their waste water
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Hello, thank you so much for the video. In response to question 3 45:57, should it be 1776.61 hours?
no
For the last problem shouldn’t the products be H2SO3 + H2O ?
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how is the cathode less positive if its supposed to be more positive then the anode?
Around 31 minutes he was talking about bringing the -1 from the denominator up to the numerator, and I was just wondering why doesn't the n also become negative?