I was utterly confused and watched so many videos yet couldn't really wrap my head around the concept. You made it seem so simple and clearly explained from the basics. I cannot thank you enough! Truly a lifesaver ❤🥺
For anyone confused on increasing the concentration of the Zn and Cu at 6:04, here's an explanation: The Anode is Zn and the Cathode is Cu: Anode: Zn was oxidized to Zn+. (The anode [Zn+] increases and is the 'product'.) Cathode: Cu+ was reduced to Cu. (The cathode [Ag+] decreases and is the 'reactant'.) Focus on the aqueous solutions to figure out which one belongs to the reactant or product side. *According to Le Chatelier's principle:* *Increasing the reactants* causes the chemical reaction to speed up because increasing the concentration of the reactants will increase the frequency of collisions between the reactants. In a sense, increasing the concentration of the reactants causes the reaction to shift to the right which increases cell potential and the flow of electrons. *To slow down the reaction, you need to do the opposite: increase the concentration of the products.* Increasing the concentration of the products causes the reaction to shift to the left which decreases the cell potential and the flow of electrons.
"The Anode is Zn and the Cathode is Cu", that is opposite what I learned in high school. Zn has extra electron, carries negative charge, so that electrode should be called cathode, right? That's the definition "cathode" from dictionary, forget about chemistry for a second. Am I wrong?
@@seanleith5312 Okay ngl, I kinda forgot most of the material from AP Chem bc I already took the test but from what I can remember, Anode = anion = negative Cathode = cation = positive That's how I remember it. Ask your teacher to make sure
@@certifiedminority I'm sorry can you please explain this point again What does 'anion' and 'cation ' refer to here? I mean both of their ions are positive zn+2 and cu+2 although we called the zinc anode and copper cathode I can't see anions
@@Malak-uu9qt do not be confused, anodes and cathodes are different from anions and cations. Anions (F-, O2-, etc) and Cations (K+, Mg2+) are atoms or molecules with positive or negative charges. Cathodes are parts of a circuit where electrons are deposited (causing reduction) and anodes provide those electrons to the circuit (causing oxidation).
Your videos are magic. This was so straighforward and made so much sense. One note, the revised AP chemistry exam, I believe, as of 2015, now requires us to know the Nernst equation.
Jose Gonzales if you want to make sure, you could check on the course description provided by the collegeboard :) secure-media (.) collegeboard (.) org/digitalServices/pdf/ap/ap-chemistry-course-and-exam-description.pdf Page says no nernst equation
I finally understood electrochemistry a bit better. My prof talks too fast in the lecture that I couldnt catch up. and reading the book is just too dry and makes me fall asleep. Your video is so straight to the point, and the video speed is perfect for me to follow. Thank you for your video!
if you are having trouble remembering where in a cell, in terms of anode and cathode, oxidation and reduction occur, just remember these 2 animals.... RED CAT and AN OX! REDuction in CAThode, ANode has OXidation then use OIL RIG (Oxidation Is Loss of e-, Reduction Is Gain of e-) to decide which half-cell is losing e- and which is gaining them! good luck on your chem guys!
Thank you so much! I'm taking my MCAT tomorrow and this vid gave me all the confidence I needed to tackle any passages with this topic!!! Very well presented :)
IDK why this has literally been the toughest concept in Chem for me to grasp. I have gone over it a billion times in my textbook and notes... watched videos and everything but still feel like i don't quite have it down 100%. Wish me luck for my exam! :) :P
***** The hard chapter of chemistry for me is the equilibrium (change in the system) part . And redox it's just seeing a table that is given and solve it the reduction potential table. The higher metal element will oxidize and it will dissolve in the solution leading to oxidation.
Oh thank you so much! my teacher spent an entire 1 hour class to teach just how the electrons moved and I still didn't get anything -.- THANK YOU SO MUCH, YOU'RE MY HERO both for biology and chemistry, too bad I study them in spanish.
Mr. Anderson - this video was AMAZINGLY AWESOME !! I actually understood the concept - and it is really fascinating!! Your slow pace made the concept so easy to understand. This is one of your best Chemistry videos, in my opinion. I am on my way to understanding Redox reactions...
I'm Back, took some time to get my life in order. I just been accepted into a Radiology school and we are learning Physics. I hope I can come to your channel for video's. YOUR SO GREAT!
I remember the Anode - Cathode to Redox relationship as LOAN. (Left Oxidation Anode Negative) Because: The *Left* Cell, Undergoes *Oxidation*, Functions as the *Andoe*, And it has the more *Negative* potential.
Girish Manjunath this looks good, though don't fall into the trap of thinking the left cell is ALWAYS the anode. It could just as easily be the right cell if you just turn the apparatus around.
Mr. Jack Parkes Don't you know about IUPAC Naming. In LOAN the left word is for Anode this means in a Rx for example Zn(s)|Zn^2+(aq) || ................ . here on left Zn as ANODE according to IUPAC
Great video, thanks a lot. My teacher used the same mnemotechnique when talking about reduction, oxidation, cathode and anode (consonants go together and vowels go together). Keep on sciencing!
OIL RIG OIL= OXIDATION IS LOSING RIG= REDUCTION IS GAININGthink of vowels oxidation = anode they both start with vowels reduction = cathode they don't start with vowels just an easy tip I remember
I think my sticking point was the function of the salt bridge. I had to research how it activates the system which helped me complete the picture. So perhaps including a comment about it would be beneficial.
Ya man. 7:30 in the morning. I was looking at what units are on the exam and I saw that electrochemistry was on it. Our teacher (60+ year old guy) forgot to teach us that. I'm so failing this shit. LOL. But honestly, I don't even give a shit about it cuz it doesn't count toward the final mark. Well, good luck I guess... because you will probably need it if you are watching this.
dude our teacher didn't teach us this shit either because we didn't have "enough time to go over it" !!! like WHAT THE FUCK? thank you and good luck to you too ! i think we all need it at this point!
WTF? Why are teachers skimping on electrochemistry? Well the damage is done and there is no way to fix it now. I've heard that electrochemistry is not a huge part of the exam tho. So it should be all right if you know the core concepts and the formulas. Anyways, good night and good luck. Gotta get up really early tomorrow. Those asshats picked the worst time for the exam.:-(
I love how I said this 4 years ago and still getting likes on it! dont worry pals i got a 4 out of 5 on the AP test XD if I can do it you all can do it !
Benardy Boen The salt bridge is present simply for the purpose of continuing the reaction. As the Zn anode is OXIDIZED, Zn2+(aq) is formed. Well, if electrons are leaving through the conductive material to the cathode, then how do we form this aqueous solution? The nitrate (NO3-), from the salt bridge, ends up forming a bond with Zn2+. (This neutralizes the charge in the anode compartment.) The same thing with the cathode, as Cu2+(aq) is REDUCED to Cu (s), Cu leaves behind its anionic portion, let's say (SO4)2-. The cationic portion of the salt bridge, Na+, will interact with (SO4)2- in order to neutralize the charge. Overall, the purpose is to neutralize accumulating charges in each compartment of the galvanic cell. When charges are sufficiently neutralized, the reaction will proceed UNTIL the anode (Zn, in this case) has fully disintegrated.
+Akihiro Ito; you probably already solved it but I just copied a part of my lab report; Without a saltbridge no voltage is detected at all. The reason for this is that the solution in the anode container would become positively charged. If this happens the electrons will stay in solution. (They will try to make the solution neutral). The opposite would happen on the side of the cathode.There would be no flow of electrons and therefore no redox reactions would take place. The salt bridge ensures the neutral charge of the solution by adding negative or positive ions to the anode and cathode solution respectively.
thanks alot sir........since 1 week i m tryin to undestand dis but all went from top of my head today i understood wat actually is happening man!!!!thank u again and i was also about to say so explain dis chapter
Very helpful, thanks. I remember that the Reduction takes place at the Cathode because it sounds like RedCat. To know which electrode gains mass you remember Fat Red Cat :P
Thank You So Much Sir...🙏🏻😍😍 Its Very Streight Forward....👍🏻& Understanding.....👍🏻👍🏻👍🏻👍🏻 So sorry Watch It Very Late But Now I Watch Your Video....👍🏻👍🏻👍🏻👍🏻👍🏻
You say that without the salt bridge no voltage will be created but I thought the salt bridge was to balance out the charge. So this would actually work without the salt bridge but only for a much shorter time?
Hello Only Nosense , Can I ask you something Do you know why zinc is oxidized, copper ions in other cups so I think it is impossible to oxidize zinc atom???
I am pretty sure it isn't 1.10 volts. The rule is Cathode+ (-anode) or .76 -(.34)=.42 as voltage difference. Or E. I am not sure why you added them like such. *_Nevermind, you had it previously set to Oxidation._*
Hai,Thanks for the video.It was helpful. I have a doubt regarding this by the way.I understand that salt bridge is Na2SO4 salt.When Oxidation happens, Zinc atom loses its 2 electron which goes to the external circuit and zn2+ ion will be in the zinc sulphate solution.Zinc ion reacts with SO4 2- ions from the salt bridge and the electrolyte would be neutral.Now in the cathode part Copper from copper sulphate solution combines with the 2 electrons from the anode and copper metal deposites on the cathode leaving soa 2- ions.This makes the electrolyte at cathode negative in charge. 1.What happens to SO4 2- ions,does it combine with Na2+ ions in the salt bridge turning the solution a mixture of Na2SO4 and Cu2SO4 solution? 2.Untill what condition does the redox reaction prolong,Is it untill zinc totally gets consumed or at a condition where there is no more Na2+ or SO4 2- ions in Salt bridge to balance the electolytes?
thanks so much for the simple video. Personally, I visualize my mnemonics, so whenever I try to recall reduction at the cathode and anode oxidation, I think of RED CAT AN OX and see a red cat walking by an ox... simpletons like me need visuals to remember all those things!
Increasing the amount of zinc would make the reaction go backwards, according to Le Chatelier's principle. And increasing amount of cu would make it go forward.
I know this is a year ago but it might help the students in the future who are also confused by this. The Anode is Zn and the Cathode is Cu: Anode: Zn was oxidized to Zn+. (The anode [Zn+] increases and is the 'product'.) Cathode: Cu+ was reduced to Cu. (The cathode [Ag+] decreases and is the 'reactant'.) Concentrate on the aqueous solutions to figure out which one belongs to the reactant or product side. According to Le Chatelier's principle: *Increasing the reactants* causes the chemical reaction to speed up because increasing the concentration of the reactants will increase the frequency of collisions between the reactants. In a sense, increasing the concentration of the reactants causes the reaction to shift to the right which increases cell potential and the flow of electrons. To do the opposite, you need to *increase the products* to slow down the reaction. Increasing the concentration of the product causes the reaction to shift to the left which decreases the cell potential and the flow of electrons.
Dear Mister Andersen As a school project I built a very simple lead-acid battery to investigate cycle fade. The capacity of my lead-acid battery decreased as the number of cycles increased, as expected. Surprisingly enough, the capacity increased after a 24 day period of deep discharge. I did the same thing three more times (so a couple of cycles followed by a long period of deep discharge) and every time the capacity had increased after the period of deep discharge. The battery did become more difficult to charge (to induce current flow a voltage of about 10 to 16 volts was necessary, just for a few seconds) and eventually it stopped working. However, I was very surprised to see that the capacity loss after a few cycles, and I was wondering whether you could enlighten me. I assume you will not have time to answer my question, but I'd greatly appreciate if you could shed some light on this issue. I have attached my results to this email, in case you are willing to take a look. Thanks in advance, Nol Duindam
Sorry...but I don't understand something...this is a galvanic cell so isn't the electrons suppose d to flow from the cathode to the anode because the anode in this case is negative and electrons always flow from the positive to the negative.... Plz respond as quick as possible
Why does adding more zinc slow the reaction and adding more copper speed up the reaction? It makes more sense to me for it to be the other way around. Also when he says slow and speed up does he mean favor the reactants or products side since we're talking about the initial and final states, not what's in between?
If you know Le Chatelier's Principle you would know that: in equilibrium if a factor which affects the state of equilibrium is changed the reaction (forward or reverse) which counteracts that change is favoured. [Zn(s) + Cu+(aq) (=> /
Anyone knows how to solve this problem and explain why choose the following answer? this question had blown my top. >< hope anyone can solve this by giving explanation... *This is a preparation of voltaic cell, which both electrodes are made in carbon, and the electrolytes in each ends of the U-tube are connected by sulfuric acid. one of the electrolyte is potassium chloride. what will be the possible electrolyte of the other end? (A) Iodine water (B) Bromine water (C) acidified potassium permanganate (IIV) solution (D) Potassium iodide solution
The zinc that is losing electrons is the zinc that is on the anode to begin with, the zinc in the solution is ionized and is not losing electrons. The zinc atoms on the anode that lose electrons go on to be ionized atoms that are released into the aqueous solution. The salt bridge has a function that Mr. Bozeman does not go in depth about, but it basically stabilizes the the concentrations of fluctuating ions in both solutions, completing the circuit.
+Gabriel Augusto Alves dos Reis hmmm, that's interesting. Tbh i gave sat a couple of days ago and in the prep book it said STP is 0C and 1 atm, while standard conditions, which is different than STP, is 25C and 1 atm. And i checked on google as well. Maybe you are confused with something else? Or maybe the Brazilian method is different. Could you maybe confirm and tell me. I would really like to know
I was utterly confused and watched so many videos yet couldn't really wrap my head around the concept. You made it seem so simple and clearly explained from the basics. I cannot thank you enough! Truly a lifesaver ❤🥺
For anyone confused on increasing the concentration of the Zn and Cu at 6:04, here's an explanation:
The Anode is Zn and the Cathode is Cu:
Anode: Zn was oxidized to Zn+. (The anode [Zn+] increases and is the 'product'.)
Cathode: Cu+ was reduced to Cu. (The cathode [Ag+] decreases and is the 'reactant'.)
Focus on the aqueous solutions to figure out which one belongs to the reactant or product side.
*According to Le Chatelier's principle:*
*Increasing the reactants* causes the chemical reaction to speed up because increasing the concentration of the reactants will increase the frequency of collisions between the reactants. In a sense, increasing the concentration of the reactants causes the reaction to shift to the right which increases cell potential and the flow of electrons.
*To slow down the reaction, you need to do the opposite: increase the concentration of the products.* Increasing the concentration of the products causes the reaction to shift to the left which decreases the cell potential and the flow of electrons.
"The Anode is Zn and the Cathode is Cu", that is opposite what I learned in high school. Zn has extra electron, carries negative charge, so that electrode should be called cathode, right? That's the definition "cathode" from dictionary, forget about chemistry for a second. Am I wrong?
@@seanleith5312 Okay ngl, I kinda forgot most of the material from AP Chem bc I already took the test but from what I can remember,
Anode = anion = negative
Cathode = cation = positive
That's how I remember it. Ask your teacher to make sure
@@certifiedminority Thank you very much
@@certifiedminority I'm sorry can you please explain this point again
What does 'anion' and 'cation ' refer to here? I mean both of their ions are positive zn+2 and cu+2 although we called the zinc anode and copper cathode I can't see anions
@@Malak-uu9qt do not be confused, anodes and cathodes are different from anions and cations. Anions (F-, O2-, etc) and Cations (K+, Mg2+) are atoms or molecules with positive or negative charges. Cathodes are parts of a circuit where electrons are deposited (causing reduction) and anodes provide those electrons to the circuit (causing oxidation).
Your videos are magic. This was so straighforward and made so much sense.
One note, the revised AP chemistry exam, I believe, as of 2015, now requires us to know the Nernst equation.
You're right. I checked with my teacher. She accidentally gave us a worksheet then told us not to do it.
Jose Gonzales if you want to make sure, you could check on the course description provided by the collegeboard :) secure-media (.) collegeboard (.) org/digitalServices/pdf/ap/ap-chemistry-course-and-exam-description.pdf Page says no nernst equation
Thanks, I'm always unsure about what it is
I finally understood electrochemistry a bit better. My prof talks too fast in the lecture that I couldnt catch up. and reading the book is just too dry and makes me fall asleep. Your video is so straight to the point, and the video speed is perfect for me to follow. Thank you for your video!
I haven't seen you in about 6 years. This review took me back to high school. Thank you for the quick review. Very helpful.
I'm from Germany and I thank you for this video. You explain it so much easier than the persons in the German videos about Electrochemistry.
if you are having trouble remembering where in a cell, in terms of anode and cathode, oxidation and reduction occur, just remember these 2 animals....
RED CAT and AN OX!
REDuction in CAThode, ANode has OXidation
then use OIL RIG (Oxidation Is Loss of e-, Reduction Is Gain of e-) to decide which half-cell is losing e- and which is gaining them! good luck on your chem guys!
Tq so much sir
thanks brett that's very useful dude
Mr.Paul Anderson was on TEDx Talks!!!!!
Way to go sir!!!!! You are the best :)
When life hands you lemons, make a lemon battery.
Alive?
Perfect clean explanation. No bull shit analogies or metaphors. Great work!
Bozeman is BOSS!!! Very helpful sir. This channel and KhanAcademy are my favourite educational UA-cam channels.
Hi
I need your help
Thank you so much! I'm taking my MCAT tomorrow and this vid gave me all the confidence I needed to tackle any passages with this topic!!! Very well presented :)
IDK why this has literally been the toughest concept in Chem for me to grasp. I have gone over it a billion times in my textbook and notes... watched videos and everything but still feel like i don't quite have it down 100%. Wish me luck for my exam! :) :P
I think redox reaction will help you to understand this. Oxidation and reduction
*****
The hard chapter of chemistry for me is the equilibrium (change in the system) part . And redox it's just seeing a table that is given and solve it the reduction potential table. The higher metal element will oxidize and it will dissolve in the solution leading to oxidation.
+Akihiro Ito Its okay she already failed her exam
Lol no I actually ended up with a 91 in the class :P
+Yasmine Xo remember OIL RIG it's a tool that helps you remember these chem terms or Leo Ger
Oh thank you so much! my teacher spent an entire 1 hour class to teach just how the electrons moved and I still didn't get anything -.- THANK YOU SO MUCH, YOU'RE MY HERO both for biology and chemistry, too bad I study them in spanish.
You deliver the concept so much better than my professor in NTU. Thank you so much.
You're the best teacher, learned alot of things in 8 minute, it was worth it❤
He is Awesome and makes you create predictions of what will occur if you change conditions in a cell.
I have read my textbook and taken notes on this chapter, literally over 20 times and it did not click until NOW! THANK YOU!!!
thank you so much for these videos, i couldn't survive chem without them!! :)
bdw E= 0.76 V is oxidation potential of Zn.. not reduction potential
its reduction potential as he said would be -0.76V
thanks man I knew something was up!
THAT IS LIKE 3 YEAR WENT U SAW THE VIDEO
Your molecular biology videos have helped me so much :)
And now you're helping me overcome my fear of chemistry. Thank you :)
Hi
I need your help
Because I have electroplating works..
Mr. Anderson - this video was AMAZINGLY AWESOME !! I actually understood the concept - and it is really fascinating!! Your slow pace made the concept so easy to understand. This is one of your best Chemistry videos, in my opinion. I am on my way to understanding Redox reactions...
I'm Back, took some time to get my life in order. I just been accepted into a Radiology school and we are learning Physics. I hope I can come to your channel for video's. YOUR SO GREAT!
I love study from your videos. They are simple and easy to understand.
I wish you were my teacher...
He doesn't treat it like it's difficult. That's why he's so good. I feel relaxed when I learn from him. :)
OMG that waterfall analogy is like magic. The cleanest way to explain that reduction potential!! Thank you!
I remember the Anode - Cathode to Redox relationship as LOAN.
(Left
Oxidation
Anode
Negative)
Because:
The *Left* Cell,
Undergoes *Oxidation*,
Functions as the *Andoe*,
And it has the more *Negative* potential.
Girish Manjunath this looks good, though don't fall into the trap of thinking the left cell is ALWAYS the anode. It could just as easily be the right cell if you just turn the apparatus around.
Jack Parkes BY CONVENTION!
Mr. Jack Parkes Don't you know about IUPAC Naming. In LOAN the left word is for Anode this means in a Rx for example Zn(s)|Zn^2+(aq) || ................ . here on left Zn as ANODE according to IUPAC
I just have to say that your videos are so clear and informative!
oxidation potential of zinc is +0.74
its reduction potential -0.74
Paul had made a mistake in the video, just fixing it.
Great video, thanks a lot. My teacher used the same mnemotechnique when talking about reduction, oxidation, cathode and anode (consonants go together and vowels go together). Keep on sciencing!
OIL RIG OIL= OXIDATION IS LOSING RIG= REDUCTION IS GAININGthink of vowels oxidation = anode they both start with vowels reduction = cathode they don't start with vowels just an easy tip I remember
You are the Savior sent by Science to rescue us students 🙌🙌🙌 thanku so much
you are the best in making mind maps
I think my sticking point was the function of the salt bridge. I had to research how it activates the system which helped me complete the picture. So perhaps including a comment about it would be beneficial.
Oh Mr Anderson also teach chemistry! I love your biology videos!
Wow thank you so much. You just broke that down SO wonderfully. That diagram really helped. Awesome vid!
-used to be confused college student
AP chem test tomorrow anyone ?
Ya man. 7:30 in the morning. I was looking at what units are on the exam and I saw that electrochemistry was on it. Our teacher (60+ year old guy) forgot to teach us that. I'm so failing this shit. LOL. But honestly, I don't even give a shit about it cuz it doesn't count toward the final mark. Well, good luck I guess... because you will probably need it if you are watching this.
dude our teacher didn't teach us this shit either because we didn't have "enough time to go over it" !!! like WHAT THE FUCK? thank you and good luck to you too ! i think we all need it at this point!
WTF? Why are teachers skimping on electrochemistry? Well the damage is done and there is no way to fix it now. I've heard that electrochemistry is not a huge part of the exam tho. So it should be all right if you know the core concepts and the formulas. Anyways, good night and good luck. Gotta get up really early tomorrow. Those asshats picked the worst time for the exam.:-(
Yup yup
I love how I said this 4 years ago and still getting likes on it! dont worry pals i got a 4 out of 5 on the AP test XD if I can do it you all can do it !
Your knowledge is absolutely impressive! Thank you for all of your videos
Thank you sir for the help of my exam
Yes
You didn't say why salt bridge is added the reason of adding salt bridge not only completing circuit,
Akihiro Ito up up!. I also want to know what is happening inside the bridge.
Benardy Boen The salt bridge is present simply for the purpose of continuing the reaction. As the Zn anode is OXIDIZED, Zn2+(aq) is formed. Well, if electrons are leaving through the conductive material to the cathode, then how do we form this aqueous solution? The nitrate (NO3-), from the salt bridge, ends up forming a bond with Zn2+. (This neutralizes the charge in the anode compartment.)
The same thing with the cathode, as Cu2+(aq) is REDUCED to Cu (s), Cu leaves behind its anionic portion, let's say (SO4)2-. The cationic portion of the salt bridge, Na+, will interact with (SO4)2- in order to neutralize the charge.
Overall, the purpose is to neutralize accumulating charges in each compartment of the galvanic cell. When charges are sufficiently neutralized, the reaction will proceed UNTIL the anode (Zn, in this case) has fully disintegrated.
+Akihiro Ito; you probably already solved it but I just copied a part of my lab report;
Without a saltbridge no voltage is detected at all. The reason for this is that the solution in the anode container would become positively charged. If this happens the electrons will stay in solution. (They will try to make the solution neutral). The opposite would happen on the side of the cathode.There would be no flow of electrons and therefore no redox reactions would take
place. The salt bridge ensures the neutral charge of the solution by adding negative or positive ions to the anode and cathode solution respectively.
He should have explained this in the video. Thanks so much. It makes sense now.
Sorka Tamwura Deeyor Great explanation man you saved me
very great simple explanation
Thank you, really benefits and clear.
How do you know what polyatomic or general atoms to use in your salt bridge?
You have saved my lil butt. Again. Thank you!!!
thanks alot sir........since 1 week i m tryin to undestand dis but all went from top of my head today i understood wat actually is happening man!!!!thank u again and i was also about to say so explain dis chapter
Very helpful, thanks. I remember that the Reduction takes place at the Cathode because it sounds like RedCat. To know which electrode gains mass you remember Fat Red Cat :P
Thank You So Much Sir...🙏🏻😍😍
Its Very Streight Forward....👍🏻& Understanding.....👍🏻👍🏻👍🏻👍🏻
So sorry Watch It Very Late But Now I Watch Your Video....👍🏻👍🏻👍🏻👍🏻👍🏻
Absolutely genius
You say that without the salt bridge no voltage will be created but I thought the salt bridge was to balance out the charge. So this would actually work without the salt bridge but only for a much shorter time?
Hello Only Nosense ,
Can I ask you something
Do you know why zinc is oxidized, copper ions in other cups so I think it is impossible to oxidize zinc atom???
ua-cam.com/video/LahawEMMvvY/v-deo.html
In the Anode, Zn oxidizes to Zn2+ not Zn+
You can NOT use Le Chatelier's principle as an explanation anymore on the AP exam. You can/should qualitatively use Nernst Eq
I still dont get why you need the salt bridge. Can someone please explain?
Terimakasih, salam, tareq
faze pizzanuke are you a nigga?
@@mcappleface8131 yes i am nasgor
I am pretty sure it isn't 1.10 volts.
The rule is Cathode+ (-anode) or .76 -(.34)=.42 as voltage difference. Or E. I am not sure why you added them like such.
*_Nevermind, you had it previously set to Oxidation._*
Because the zinc potential is actualy negative, therefore you have to add them together ;) :)
Should not it read negative .76 V since Zn is less precious, and it would correctly be positive .34 V for the Copper?
how do you know which way electricity will flow ? should one plate be thicker than the other ? and why ?
I am very happy for this great and informative lecture,God bless you.
We did the lemon thing in physics class last year (Ontario grade11)!
RED CAT
reduction at the cathode
Hai,Thanks for the video.It was helpful.
I have a doubt regarding this by the way.I understand that salt bridge is Na2SO4 salt.When Oxidation happens, Zinc atom loses its 2 electron which goes to the external circuit and zn2+ ion will be in the zinc sulphate solution.Zinc ion reacts with SO4 2- ions from the salt bridge and the electrolyte would be neutral.Now in the cathode part Copper from copper sulphate solution combines with the 2 electrons from the anode and copper metal deposites on the cathode leaving soa 2- ions.This makes the electrolyte at cathode negative in charge.
1.What happens to SO4 2- ions,does it combine with Na2+ ions in the salt bridge turning the solution a mixture of Na2SO4 and Cu2SO4 solution?
2.Untill what condition does the redox reaction prolong,Is it untill zinc totally gets consumed or at a condition where there is no more Na2+ or SO4 2- ions in Salt bridge to balance the electolytes?
excellent .Tell us more about reduction/ oxidation potential
why in Daniel cell the anode is shown negative
and cathode is shown positive.
thanks so much for the simple video. Personally, I visualize my mnemonics, so whenever I try to recall reduction at the cathode and anode oxidation, I think of RED CAT AN OX and see a red cat walking by an ox... simpletons like me need visuals to remember all those things!
I don't understand why increasing the amount of Zn would slow the solution, and increasing the amount of copper would speed it up .
Increasing the amount of zinc would make the reaction go backwards, according to Le Chatelier's principle. And increasing amount of cu would make it go forward.
I know this is a year ago but it might help the students in the future who are also confused by this.
The Anode is Zn and the Cathode is Cu:
Anode: Zn was oxidized to Zn+. (The anode [Zn+] increases and is the 'product'.)
Cathode: Cu+ was reduced to Cu. (The cathode [Ag+] decreases and is the 'reactant'.)
Concentrate on the aqueous solutions to figure out which one belongs to the reactant or product side.
According to Le Chatelier's principle:
*Increasing the reactants* causes the chemical reaction to speed up because increasing the concentration of the reactants will increase the frequency of collisions between the reactants. In a sense, increasing the concentration of the reactants causes the reaction to shift to the right which increases cell potential and the flow of electrons.
To do the opposite, you need to *increase the products* to slow down the reaction. Increasing the concentration of the product causes the reaction to shift to the left which decreases the cell potential and the flow of electrons.
pls make MCAT videos, this helped me so much
Are the factors that increase the voltage in a glavanic cell the same factors that would increase voltage of an electrolytic cell (battery)???
Thank you very much)) It is really helpful)
Thanks for the vidios they are very helpful.
LEO says GER
Loosing Electrons is Oxidation
Gaining Electrons is Reduction
losing* ;)
Aight
OILRIG.............Oxidation-ion lose...........Reduction-ion gain
OILRIG
yo you took Birkenfeld's class?????
@6:15 why did he say that if we increase the Zn in the solution, the reaction will slow down?
Because they are of positive chargé and Will result in there being a Decreases flow of electrons
thank you Sir
honestly needed this! thanks so much, you are appreciateddd
thanks for clearing my concepts
thanks for the great video!! :)
LEO the lion goes GER
Loss of Electrons is Oxidation / Gain of Electrons is Reduction
Dear Mister Andersen
As a school project I built a very simple lead-acid battery to investigate cycle fade.
The capacity of my lead-acid battery decreased as the number of cycles increased, as expected. Surprisingly enough, the capacity increased after a 24 day period of deep discharge. I did the same thing three more times (so a couple of cycles followed by a long period of deep discharge) and every time the capacity had increased after the period of deep discharge.
The battery did become more difficult to charge (to induce current flow a voltage of about 10 to 16 volts was necessary, just for a few seconds) and eventually it stopped working. However, I was very surprised to see that the capacity loss after a few cycles, and I was wondering whether you could enlighten me.
I assume you will not have time to answer my question, but I'd greatly appreciate if you could shed some light on this issue. I have attached my results to this email, in case you are willing to take a look.
Thanks in advance,
Nol Duindam
I don't discus any cell formula
Why did I think the diagram was gunna break out in a dance or something at 1:30 ??
very nice video
awesome video .........
Only passed my chem test because of these videos!!
you mean when we put Zn into Zn2+ solution ---> naturally,we will have electron on the mettal bar....i still do not understand that point ???
thanks for the lesson :)
Very nice explan
why does adding zinc decrease the potential???
Could someone please explain what drives the solid zinc to move into solution spontaneously, as mentioned at 5:30?
I want all link of electrochemical cell chapter.... its too tough .... plz forward link plzzz
Sorry...but I don't understand something...this is a galvanic cell so isn't the electrons suppose d to flow from the cathode to the anode because the anode in this case is negative and electrons always flow from the positive to the negative....
Plz respond as quick as possible
Why does adding more zinc slow the reaction and adding more copper speed up the reaction? It makes more sense to me for it to be the other way around. Also when he says slow and speed up does he mean favor the reactants or products side since we're talking about the initial and final states, not what's in between?
If you know Le Chatelier's Principle you would know that: in equilibrium if a factor which affects the state of equilibrium is changed the reaction (forward or reverse) which counteracts that change is favoured.
[Zn(s) + Cu+(aq) (=> /
Seriously, you are awesome.
very good!👍
Very good..
Thanks a lot
Anyone knows how to solve this problem and explain why choose the following answer? this question had blown my top. >< hope anyone can solve this by giving explanation...
*This is a preparation of voltaic cell, which both electrodes are made in carbon, and the electrolytes in each ends of the U-tube are connected by sulfuric acid. one of the electrolyte is potassium chloride. what will be the possible electrolyte of the other end?
(A) Iodine water (B) Bromine water (C) acidified potassium permanganate (IIV) solution (D) Potassium iodide solution
greetings bezeman! i kind wonder why the electrons lost by zinc dont go to the bridge first? how could them make a choice? thx alot
The zinc that is losing electrons is the zinc that is on the anode to begin with, the zinc in the solution is ionized and is not losing electrons. The zinc atoms on the anode that lose electrons go on to be ionized atoms that are released into the aqueous solution. The salt bridge has a function that Mr. Bozeman does not go in depth about, but it basically stabilizes the the concentrations of fluctuating ions in both solutions, completing the circuit.
Galvanic cells actually took me awhile to get the hand of.
I wish you were my physical chemistry professor
At 2:04, he said STP (standard temp. and pressure),
but isn't STP different from standard conditions (1 M)? Or are they the same thing?
Janice Ji Standard conditions means 1M solutions, reacting under STP.
:D
+Girish Manjunath not true, STP is 0 Celsius while standard condition is room temperature(25 Celsius)
.
Muneeb Khan Sorry, my bad, STP is 0C and 1bar, not 25C and 1atm, I got confused... XP
+Muneeb Khan i dont know where you guys live, but in brazil universities stp is 1atm/25º
+Gabriel Augusto Alves dos Reis hmmm, that's interesting. Tbh i gave sat a couple of days ago and in the prep book it said STP is 0C and 1 atm, while standard conditions, which is different than STP, is 25C and 1 atm. And i checked on google as well. Maybe you are confused with something else? Or maybe the Brazilian method is different. Could you maybe confirm and tell me. I would really like to know
What is the role of electrolyte in it??
Excellent!. Sir Will u plz explain why Anode has negative charge in galvanic cell?
So can we increase the amount of silver at the cost of Zn?