Standard Reduction Potentials of Half Reactions - Electrochemistry

This chemistry video tutorial provides a basic introduction into standard reduction potentials of half reactions. It explains how to identify the strongest oxidizing agent and the strongest reducing agent. Oxidizing agents are found on the left side of the reduction reaction and reducing agents are found on the right side of the reduction. Oxidizing agents have a strong affinity for electrons and reducing agents have a strong desire to give away electrons. This electrochemistry has plenty of questions and practice problems relating to standard reduction potentials.
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...
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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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[@raajkumar8039]

E+ spon in Forward Direction
Non-spon in Reverse Direction.
3:34 - By Adjusting the pH we csn adjust the Cell Potential of the Reaction.
4:45 - the one with higher cell potential will act as Better oxidizing or reducing Agent
6:56 - Anything that's neutral/positively charged can behave as Oxidizing agent
- Neutral/Negatively charged can behave as reducing Agent.

[@raajkumar8039]

Pardon my notes :D

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[@Engr9]

11:01 Metals and negatively charged ions tend to be reducing agents.
Nonmentals and positively charged ions tend to be oxidizing agents

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idk why but you and my prof in analytical chem explain lesson in the same sequence (sometimes the same examples are given as well)

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Thank you for the videos! There's only one thing that would make the videos even better(at least for me) is that some words aren't clear enough I think because you say them quickly. I hear south potential in this one for example

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[@MegaPruddy]

In 7:10, How can it be if an is negatively charge it has the ability to give away electrons?

[@tonyaamini8876]

Is there a way to calculate the cell potential

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Nice

[@tanyayasmin6101]

is cu+(aq) have low reduction potential ??

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The word choice is quite enticing (pun intended)

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Sir how can we solve to get the volts or E°, if we don't have the table?

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[@pompom2621]

When the e- is on the right side of the equation isn’t that supposed to be oxidation? The video said it was reduction so I’m even more confused now.

[@mirjanavrdoljak899]

Why is the standard electrode potential always expressed for the process of reduction rather than oxidation? Thank you

[@willieriley6079]

Thats just how the tables are made

[@mirjanavrdoljak899]

@@willieriley6079 why thats? why they are not made for the oxidation process- why exactly for the reduction process? thank you

[@willieriley6079]

Mirjana Vrdoljak it’s more useful i suppose because electrons flow spontaneously from something being oxidized to something being reduced as in a galvanic cell like a battery and it works with Nernst equation or the delta G= -nFE equation where positive potential E would make for a spontaneous reaction due to -G. Also just flipping the reaction itself is oxidation so it’s not too difficult, but my guess is the reduction helps more for knowledge on practical uses.

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👍

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Zn 2- ion (never heard of such thing) 😂😂😂😂

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“Now let’s see if you were paying attention” *immediately restarts video*

[@adrikaafrin]

well, aren't these reactions reversible?!