Electrochemistry - Free Formula Sheet: bit.ly/3NLeylq Final Exams and Video Playlists: www.video-tutor.net/ Chemistry PDF Worksheets: www.video-tutor.net/chemistry-basic-introduction.html Next Video: th-cam.com/video/S9frctwDyL0/w-d-xo.html
Wish I would have found your videos sooner. I got a C and and D on my first two gen chem 2 exams. Hoping your videos help me get a better grade on the finals! My teacher has been so bad at teaching and you're honestly amazing!
These videos have been so incredibly helpful! I don't remember if I took chemistry in HS. Ha. that long ago. Currently, I am taking an accelerated pre-req general chemistry I and II courses online and I would be so lost without these videos. You and another tutor on TH-cam are my favs! Thank you Thank you! Keep up the great work.
Hello sir how are? Actually your lesson have really started improving my studies, however i may want to know what determies a metal to be at the anode or cathode whe drowing a galvanic cell? Thanks very much
the lowest or more negative SRP value tends to be the anode while the more positive one tends more to be the cathode in a galvanic cell, if only the half-reactions are given
Anode(+ electrode ) attracts anions ( - charge ions ). Cathode (- electrode ) attracts cations (+ charge ions). Metals are usually positive charged so they usually go to the cathode.
Hi guys, I would like to ask for help with electroplating, specifically nickel and copper plating. I need to coat some small pieces of both black steel and stainless steel. I bought nickel sulfate and copper sulfate and pure nickel (99.9%) for this purpose. As the copper anode, I used the electric wire. I dissolved nickel sulfate and copper sulfate separately in two containers in hot distilled water (I did not weigh the water to sulfate ratio), connected pure nickel (or copper wire in a second way) to the anode (+) and my steel object to the cathode (-) and set three volts on the source (I also tried some other voltage setting between 2 volts and 6 volts). My steel peace was degreased (I used both strongly degreasing alkaline bath or simply dishwashing detergent). My results in the case of nickel plating (for both black and stainless steel): steel pieces are coated by the very thin BLACK layer that can be cleaned with a sponge for dishes under running water. My results in the case of copper plating (I tried only black steel): steel pieces are coated by a rapidly increasing copper layer (I do not need to turn on the power source, just dip the steel object in the copper sulfate solution, and the cooper appears on the surface). Unfortunately, this cooper coat can be simply removed under running water only by rubbing the hand. Copper is not firmly attached to the steel. Can you help me where I do something wrong? I will be very grateful for any advice.
It depends on the person. My chem teacher does it both ways and makes us choose. It’s easier to do it with what I call unit conversions so you see where you messed up bc to use farraday, you gotta convert before using it so sometimes it’s just easier in one go🤷♀️
Electrochemistry - Free Formula Sheet: bit.ly/3NLeylq
Final Exams and Video Playlists: www.video-tutor.net/
Chemistry PDF Worksheets: www.video-tutor.net/chemistry-basic-introduction.html
Next Video: th-cam.com/video/S9frctwDyL0/w-d-xo.html
God knows, you're more of a lecturer than my actual lectures have been. I study with so many of your videos. Please keep up the good work
Wish I would have found your videos sooner. I got a C and and D on my first two gen chem 2 exams. Hoping your videos help me get a better grade on the finals! My teacher has been so bad at teaching and you're honestly amazing!
Best chemistry channel on the platform
The way you are writing your equations up is so beautiful. I never saw something like that. thank you for showing me how to do it
These videos have been so incredibly helpful! I don't remember if I took chemistry in HS. Ha. that long ago. Currently, I am taking an accelerated pre-req general chemistry I and II courses online and I would be so lost without these videos. You and another tutor on TH-cam are my favs! Thank you Thank you! Keep up the great work.
organic chemistry tutor is the goat
You are truly God sent. Keep up the good work.
Your tutorials are great! Very helpful for lots of topics!
this man is my savior
Can you please tackle about Faraday's laws. This will be very helpful :) Thank you.
Thanks!
You, good sir, are going directly to heaven
well done .i appreciate from INDIA
You are doing a great job
thank you very much i practiced myself on this
you are the goat bro
Awesome lecturer
Thank you so much, you're life saver
Very good lecture. Thanks.
Pealse we need Faraday's first and second law explanation .
Thank you, this helped a lot
In last question how you write the equation can you please explain
Thank you this helped me a lot
What is the exact formula we're using here? Can anyone tell?
m = itM/zf
m = mass
I = current
M = molar mass
Z = number of moles
F= Faraday constant
The t is for time?
Hello sir how are? Actually your lesson have really started improving my studies, however i may want to know what determies a metal to be at the anode or cathode whe drowing a galvanic cell? Thanks very much
💀💀💀 might be too late but it is determined by which metal is being oxidized, and the metal that is being oxidized will be the anode
the lowest or more negative SRP value tends to be the anode while the more positive one tends more to be the cathode in a galvanic cell, if only the half-reactions are given
Anode(+ electrode ) attracts anions ( - charge ions ).
Cathode (- electrode ) attracts cations (+ charge ions).
Metals are usually positive charged so they usually go to the cathode.
Thank you so much!!
lifesaver! tysm!
This has to be the only video I have watched from you, that I couldn’t understand. Im sorry
You just have to be familiar with some basics.
Hi guys,
I would like to ask for help with electroplating, specifically nickel and copper plating. I need to coat some small pieces of both black steel and stainless steel. I bought nickel sulfate and copper sulfate and pure nickel (99.9%) for this purpose. As the copper anode, I used the electric wire.
I dissolved nickel sulfate and copper sulfate separately in two containers in hot distilled water (I did not weigh the water to sulfate ratio), connected pure nickel (or copper wire in a second way) to the anode (+) and my steel object to the cathode (-) and set three volts on the source (I also tried some other voltage setting between 2 volts and 6 volts). My steel peace was degreased (I used both strongly degreasing alkaline bath or simply dishwashing detergent).
My results in the case of nickel plating (for both black and stainless steel): steel pieces are coated by the very thin BLACK layer that can be cleaned with a sponge for dishes under running water.
My results in the case of copper plating (I tried only black steel): steel pieces are coated by a rapidly increasing copper layer (I do not need to turn on the power source, just dip the steel object in the copper sulfate solution, and the cooper appears on the surface). Unfortunately, this cooper coat can be simply removed under running water only by rubbing the hand. Copper is not firmly attached to the steel.
Can you help me where I do something wrong? I will be very grateful for any advice.
u good after 3 years?
Thanks a lot bro
Your puting all the calculations in one step and i cant keep up, could you please break it down more?
Sir please give us specific resistanc, equivalent conductance, molar conductance
Way way over thinking it. You lost me at the beginning. U are to smart for me
Thanks
College is no longer necessary
But im learning this in highschool.-.
@@tensor5113 where do you live and how old were you when you learned this?
@@azizahkasim5267 california while I was 16
@@tensor5113 wow! you're so smart. Good luck in high school!
How do you know that copper is 2+? Couldn't it be 3+, too?
and the surface of the piece to be plated never intervenes?
This explanation is not very comprehensive in my opinion, I don't think the solving process needs to be this complex
Use second Faraday's law: m=(ItM)/(zF). I is current, t is time, M is molar mass, z are the exchanged electrons, F is constant, m is the mass plated
What asspull
@@stepanbmwthis was honestly so helpful thank u sm
A simplified explanation is this
Moles (of substance formed)=
(amps× time(s))/
(n (electrons in half reaction)×96500C/mol)
It looks much neater on 📃
It depends on the person. My chem teacher does it both ways and makes us choose. It’s easier to do it with what I call unit conversions so you see where you messed up bc to use farraday, you gotta convert before using it so sometimes it’s just easier in one go🤷♀️
Can someone comment some galvanizing iron by zinc by dipping question problem with answer. Plssss.
Thank youuuuuu
how to know how many mol of electron a certain element has?
Look at their redox reactions on an electrochemical series.
THANKSSS
I LOVE YOU
huh, my reference book puts 1 mol e- =96500 C
Where do you teach? I wanna see if I can enroll.
But mole is 196500
Ah yes, 1L=1000mL
midterm in 10 hours
😮❤❤❤❤
my professor , is the actual worst theses vids and the text i how I learn