Cell Potential Problems - Electrochemistry

[@TheOrganicChemistryTutor]

Electrochemistry - Free Formula Sheet: bit.ly/3NLeylq Chemistry 2 Final Exam Review: kzbin.info/www/bejne/ooTQe4FnlNqJpqs Chemistry PDF Worksheets: www.video-tutor.net/chemistry-basic-introduction.html Next Video: kzbin.info/www/bejne/n4jUhoqtrrWeidU

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[@Feyangel23]

For anyone wondering why at 7:40 the answer is -2.20V it's because electrolytic cells can have negative cell potentials which is the difference between galvonic cells. When electrolytic cells have negative cell potential values they need energy to run. It's like when your smartphone is dead; you need to recharge it first before it can run again

[@starsuperville6863]

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[@antoniojosiahphilipm.7817]

How did u get -2.20V at problem 3?

[@happy8871]

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[@tbdrosa8542]

another neat way to determine which cell potential is "flipped" is which is more negative. The more negative a cell potential is, the more it wishes to be oxidized. And when we oxidize reactions in problems similar to these we will flip the reaction, which also can flip the sign to its corresponding reduction potential

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[@georgesadler7830]

Professor Organic Chemistry Tutor, thank you for showing How to analyze and calculate cell potential of a galvanic cell/ electrolytic cell in AP/General Chemistry. In this video, the examples are simple to follow and understand from start to finish. This is an error free video/lecture on KZbin TV with the Organic Chemistry Tutor.

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[@sumaiyarashid8930]

true dat my teacher just confused me so much that i had to revisit the whole thing again

[@arexqui625]

In Standard cell potential don't we subtract the cell potential of cathode from anode as per formula?

[@shubhamsinghhh99]

Bkr video h nhi hai isko knowledge

[@chisomovuegbe4248]

Mohammad nasir you do, but he reversed one of the reactions, that’s why he still got the correct answer despite adding them.

[@manishbarnwal3816]

@@shubhamsinghhh99 I think you should check yourself before accusing him.

[@jerymarschmid6176]

yeap it should, that's how is shown on the books

[@thabangmoloi1553]

His half rxn are standard hence he can choose to reverse the other one

[@arielwise9664]

what do you do when you're not told if it's electrolytic or galvanic?

[@JulianHernandez-bt7il]

"A standard cell potential has to be positive" can't believe my professor never mentioned that in lecture man haha

[@avationmusic]

Keep in mind when he says that it has to be positive, he means the overall potential for the entire cell, and it only applies to galvanic cells. Electrolytic cells can be negative because they are powered by an external source. You can also use the value of the cell potential to determine if the reaction will be in equilibrium (Ecell = 0) or if it’s spontaneous (Ecell = positive) or non-spontaneous (Ecell = negative). Hopefully you knew this already but I’m adding it just in case :)

[@AverageMED]

@@avationmusic can an electrolytic cell be positive?? I am having a hard time wondering why they ever would be

[@user-pr5py8cw9x]

@@AverageMED He's wrong. An electrolytic cell, by definition, has a negative Ecell. Always negative. Never positive. First time I've seen him make a big mistake in a video.

[@AverageMED]

@@user-pr5py8cw9x yeah i was gonna say by definition it has to be negative

[@sneha3927]

Explanation was too simple.... Thanks 😊

[@CaptainKanundrum]

Thank you so much for this video, it is exactly what I was looking for! One question: for cases like Ag/Mg reaction, why does multiplying the Ag equation by 2 not change the cell potential at all? I keep thinking that if I have to move twice as many electrons, the potential should double.

[@arhamralam]

Cell potential is an intensive property, so it will not change even if the number of moles vary.

[@xii-cb.s.gokulakannan1945]

hi dude the basic thing of this chapter is electrode potential do not change with how many moles , pressure , temperature you add the ep donot change . i think my answer would clear your doubt .

[@srinuchandaka3959]

Thank you!!! *Organic Chemistry Tutor*

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[@davidcherilus9112]

Can anyone explain equation 3 ? Thank you. In contrast to a galvanic cell,the most positive standard reduction half reaction within an electrolytic cell is the one that experiences oxidation. With that in mind, Why did he reverse iron half reaction and not the Br half reaction (where Br would be our anode and Fe be our cathode? Ered of cathode - E red of anode.

[@catastrophicdemon949]

Br is the one receiving the electron therefore it is a reduction and Fe is losing electron therefore it’s a oxidation. Knowing that reduction is cathode and oxidation is anode. Using the formula Ered-Eox or Ecathode - Eanode = 1.09-(0.77) which is 0.32

[@ShubhraShandilya29]

Explained wonderfully! Thanks!!

[@somasch7552]

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[@kashrathore3146]

How did u get -2.20 ..I got +2.20 in the last question

[@mohammadrezasharghi8648]

In an electrolytic cell, you have to put in energy to do the electrolysis, so Gibbs free energy is positive here, which means cell potential needs to be negative, not positive.

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[@pydipaparao5379]

should we multiply the E°cell value when equation is being multiplied?

[@TheKennethfilm]

No since the standard potential is in volts and not in volts/mole.

[@7dnein944]

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I can’t believe this appeared after just throwing such question yesterday during chemistry exams 😢

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[@atttomole]

Interesting. It’s a bit confusing when it comes to the redox flow battery. Can you do it for iron redox flow battery reactions.

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[@themaninred7352]

Hi question, does molarity of the substances affect the cell potential?

[@jarodhans3758]

yes it does. for calculating cell potential in standard conditions (1M) use the method in this video. for concentrations other than 1M use nernst equation

[@zoudek123]

In 10:56, +109, pls tell me how to get that number..

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[@ab123tube4]

Great.please make video how to affect using active and inert electrode on the product of electrolysis

[@BrownCookieBoy]

First you say the cell potential has to be positive, then you introduce a nonspontaneous reaction (were the potential is negative) without explaining. Im confused. So i wouldve had the wrong answer if i flipped the Standard for aluminum so i could do 1,66 - 0,535?

[@giordicsaga]

same here! XP

[@iubescman]

for galvanic cell, that's the rule that it must be positive. in electrolytic cell it can be either

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[@sanchitbolinjkar8291]

Electrode potential is an intensive property and non additive in nature so we can't directly add it the way you did. Instead what we have to do is add all the reactions and equate it's Gibbs free energy to the final free energy. Could you pls solve this confusion for me?

[@moonandtanu7591]

Yea thats what im thinking

[@lanercat36]

Oohhh!!! I get it!! Light bulb. Thank you so much!!

[@ethioupdatedinfo.]

On question 3) (7:35) you don't multiply Fe^2+ potential by two. So the overall result should be -0.45v not +0.32v. If this is the answer why galvanic cell result negative?

[@nahuelfernandez4190]

because its asking for an electrolytic cell.

[@nurulhdm]

Question- why the volts are added together inside of subtracting it? Wouldnt you be incorporating based on the following emf formula E cell= E cathode - E anode instead?

[@ritapatel9246]

This is awesome way to understand... Thanks👍👍👌👌

[@venusz6134]

hmm I'm not quite understanding how he got +0.21V for Q2. After reversing the iron's rxn, it becomes an oxidation (anode) with E= +0.44. So should it be: E cell = E cat - E ano = -0.23 - 0.44 which is

[@sandeepsammy9480]

Even I have the same doudt and going through the comments...so that anyone can reply me .

[@sandeepsammy9480]

If your doudt has clarified .. can you please tell ?

[@venusz6134]

​@@sandeepsammy9480 Sure thing. For this question, it'd be helpful to arrange the half-rxns in the decreasing order of standard cell potential values - we will have Ni (-0.23V) then Fe (-0,44V) so Ni+2 rxn is reduction (cathode) and Fe+2 is oxidation (anode). The formula (Cathode - Anode) works according to the standard potential values of reduction half-rxn. Thus, since anode = -0.44, Cathode - Anode = -0.23 - (-0.44) = 0.23 + 0.44. Hope this helps :)

[@venusz6134]

@@sandeepsammy9480 Also it's a galvanic cell meaning Cathode - Anode always > 0

[@sandeepsammy9480]

@@venusz6134 thankyou ...I understood ..thanks for the clarification

[@ridhima1933]

Thank u so much sir, u cleared my confusion

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[@Bohnr]

I always have to speed these up, but good stuff

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[@adinahojda6669]

when we calculate the cell potential we have to do subtraction. The formula is cathode - anode. In the first example you added the values and now i am confused.

[@ayushdudhani]

In that formula we use reducation potential where as he used oxidation and red potential respectively

[@allandumagay9908]

Bro +0.80-(-2.37)=+0.80+(2.37) Still the same bro.

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[@govindarajuankadala8563]

Best explanation

[@sajidmehmood6976]

Dont you think when we subtract one from other with opposite charge the net result with sign of those which is larger term...as you did in case of secnd e.g ...suggest me please

[@sajidmehmood6976]

As in Ni and Fe eg. The net sign is negatve... I have read this eg in another book with Ni used as oxidation

[@nathanmulopo9366]

@@sajidmehmood6976 If Ni is used as oxidation it's wrong cause with half - reactions, one half - reaction must be reduced and the other oxidized . Both of them can't be oxidized. Fe is already oxidized

[@lizardis89]

I learned in class the formula for ecell was to subtract ecathode and eanode? Can you explain why you are adding them?

[@101nevergiveup]

This is the same problem I'm facing 😭

[@atlma2]

Should the cell potential for electrolytic cells always be negative (so deltaG is +) since its nonspontaneous via the equation G = -nFE?

[@johnhopley154]

yes my same thoughts. especially for the Br2 2Fe2+ one he does at like 7:30

[@antoniojosiahphilipm.7817]

Saeemm

[@brennan7846]

I just wanted to know if the balancing of the electrons changed the cell potential for my homework. Thankfully I have found somewhere where it says that it does not change. Where else can I find the answer to this question? Like actually I was surfing this channels videos to find this answer.

[@bbboyyy51]

Please tell me why souldn't we need to balance the last example?

[@rosey5357]

omgg thank you so much! This literally helped me alot!

[@stevencheng7997]

10:14 isn't it -1.12 , because e cell= e reduction - e oxidation??? I am so confused

[@tomato7453]

might be a little late, but its -2.2 because its not a galvanic cell. So the value can be negative. He added the cell potential for both (like in the others). Both equations work but the addition is when you are switching around the half reactions (like in the video where he flips a half reaction and the V is flipped in turn)

[@brianreyes5831]

thanks for always making it all seem easy :))

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Wow! Thanks man you're helping me alot ❤🙏

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I wanna hug and kiss this guy. Thank you so much!

[@lost_saint.]

5:51 how did you get those cell potentials

[@aliyaiffat5217]

Forgalvanic cell cell potential hs to be positive. For electrolytic cell it can be negative positive or zero.

[@nurislamshimul5402]

clear lecture.... thank u

[@biancafrancis7788]

how did you come up with the reduction potentials?

[@useful-__]

Sorry I need clearification on problem 3 as I think you didn't need to change the sign of the 0.77V to negative as the equations were in order.

[@johnnyzheng423]

An easier and quicker way is looking at the electric potentials of both half reactions and picking the largest electric potential. That will be your Ecathode , so you can subtract that with the lower electric potential (your Eanode) to get your overall cell potential. For example, for #1 you pick the 0.8V since it is the larger number and subtract that with -2.37V which will give you 3.17V.

[@sunny11097ify]

wait, isn't getting the cell potential of a galvanic cell done in a way in that, E(oxidation)-E(reduction)? And it seems like we do not gave to change the signs when flipping the equations around....

[@ahmedader4283]

Thankz 😭😰 u saved me

[@pelebrapsgp]

Do they often give equations along side😢.Here at my school you don't dare expect any cell equation💔. Please do a video for assigning which one should be oxidized or reduced when two elements are under consideration. Or send me a link if it is already available . That is just my challenge presently😢

[@sumaiyarashid8930]

this video was helpful

[@mishal81]

thank you sm :) god bless u. sending love your way

[@alphajohnalbert4517]

Where did they get the value of Voltage?

[@xtiiin4467]

In your second example, why did you reverse Fe and not Ni?

[@nathanmuni3745]

How do we know which reaction we have to reverse??? Either one or two 🤔🤔

[@omsingharjit]

Why cell potential of lead acid battery is 2volt if lead and sulpher potential is much lower ????

[@Fifi00416]

i was soooo confused, thank you sooooo much

[@khnithhgor9698]

when the electrons are present on the same side then which reaction is to be inversed and on what basis?

[@andrewquintana2068]

If a galvanic cell, invert the reaction that will result in a positive E. If an electrolytic cell, it depends what they are looking for. The "E" can be negative, positive, or zero. Thus it doesn't matter which you invert.

[@jameschem]

The question 4 was kinda weird to me, hope you could explain more

[@binodanandbipin5960]

Do we have to remember the data as you have shown in example 3..

[@fable9958]

Question 3 is wrong. It states that its an electrolytic cell but has a positive value for standard potential value. That will result in negative value for delta G meaning its spontaneous. Electrolytic cells are supposed to be non spontaneous. Maybe that question should I have stated that is a voltaic/galvanic cell question.

[@charitydoeses]

But the last examples answer doesn't make sense because you said the Ecell value should always be positive?? Help

[@evwerenisaacoghenenyerhovw232]

Sir , please I'm confused..... Is E cell= Ereduction - E oxidation How come did u just add together instead of subtracting please explain cos I'm kinda confused

[@JohnMcCaine-oo2uo]

Both ways are correct, it depends on what you've been taught.

[@evwerenisaacoghenenyerhovw232]

It didn't gave me same answer sir

[@JohnMcCaine-oo2uo]

@@evwerenisaacoghenenyerhovw232 Have you tried to check if the oxidation sign is supposed to be reversed or not? + or -

[@passthejay]

Subtracting a positive number is the same as adding a negative number

[@anonimuselle]

i dont understand?? i thought you dont reverse the signs of Ecathode and Eanode, you use reduction potentials directly in the formula