Electrochemical cells
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- เผยแพร่เมื่อ 2 ก.ค. 2024
- Electrochemical cells is where you put naughty electrochemicals! Sorry! This video will show how you combine half cells to make full cells including the correct cell representation, the role of the salt bridge, and calculating the electrode potential of the cell.
People like these who give free time of their own to provide students/fools like us some tuition and guidance makes me want to be a better student. Love your vids
Your videos are excellent Chris! Please continue making them. They are so helpful I am going to suggest you receive the Hawking Medal for Science Communication.
+James Barker Thanks very much for your support! I heard about the medal just before Christmas. I hardly think my little videos will get anything like that though. Ha! I think the idea that Hawking has created this award is brilliant! I am a strong advocate of communicating science to the public, it plays a big role in all our lives and shouldn't be reserved for the minority. 😉
This topic is actually making sense now and it's getting interesting! Woo thanks Chris.
+Rhea Jain You're very welcome! I like this topic too! Must students hate it, I really don't know why?!
Your videos are very helpful, thank you for putting in the hard work and providing us with free Chemistry tuition
Thanks again, you deserve an award
+russel johnson No problem at all! As long as the vids help, that's the main thing.
Makes way more sense now thanks!! You make chemistry a little more bearable!
Wow that was brilliant! I felt hopeless about electrochemistry before this video because it's past midnight and I'd forgotten the whole topic but now I feel all set for tomorrow's A level chemistry mocks! Thanks Chris!
Sir you're a lifesaver!! 😍
2019 and im still passing chemistry thanks to chris
THANK YOU SOOO MUCH FOR THIS! I LOVE YOUR CHANNEL. Love from 🇧🇩
nicely explained!! Thanks a lot!
Wow you made this seem so uncomplicated. Thank you so much!
You're welcome!
THIS VIDEO WAS SO GOOD. I FINALLY GET IT. THANK YOU SO MUCH.
Your videos save my a** through ALevel thank you ever so much❤️❤️❤️❤️❤️
Thank you Chris you don't know how muh you're changing my grades lol, it's just explained so clearly !!!!!!
your videos are so helpful!! thank you so much!!
If you were given two reduction equations and you need to flip one so it is the oxidation equation of one of the cells, do you have to flip the sign of the E naught value?
I hope this makes sense!
Yes. You just flip the equation. Hope this helps.
I really love your videos, I understand waayyyy more, I was hoping you could make a small video answering question number 4c 9701/41/M/J/15 and explaining the answers. Please ☺
Thanks. Have a new born now so finding it tough to do new videos in the short term. So pleased the videos are helping though! Good luck with your exams!
Thanks.Great video. For the last calculation you did, does the number of electrons not affect the electrode potential calculation? I thought since the +0.77 reaction only had one electron you would have to multiply its value by two to get 1.54?
Can anyone help with that?
Thank you
Really helpful as always
I'm slightly confused so i would greatly appreciate some clarification:
in eg galvanic cell Zn and Cu
if a voltmeter is connected since it has very high resistance do electrons still flow?
or
do equilibrium reactions become established and the one is just *more* oxidized than the other ?
if there's a wire it makes sense since elections will flow from anode to cathode
I'm a bit confused. When drawing a cell diagram when do you need the Pt (s)?? What if the electrodes you are using are not platinum electrodes say copper and zinc.
+Rhea Jain Yes you only use Pt when you are using a solution that doesn't have a solid, conductive atomic version of the ion. E.g. H+ solution would have an atomic equivalent of H2. Now H2 is not a solid so can't be used as an electrode, we have to use an inert, conductive metal in it's place hence the use of Pt. Using Cu2+ and Zn2+ means we can use Cu and Zn respectively. These are conductive solids and so can be used as electrodes. No need to use Pt thankfully! Would make cells very expensive!
Deserves more views
muchas gracias por todo.
Very helpful
Thank you!!
For an Fe2+ and Fe3+ half cell, why can’t you use a Fe solid electrode?
Thank you a lot !
Glad it helped
Great video. If Ecell is negative, the reaction will not happen but how would this situation occur?
so the anode is the negative electorde
Mast h