Talk:Galvanic cell

message: Does anybody notice that in the half ionic equation for the ionization of zinc in the cell, that should be:
            Zn → Zn+2 + 2e-
Zinc would lose electrons more readily than Copper as it has a higher position in the electronchemical series(E.C.S.).Narold 13:59, 6 February 2007 (UTC)
thread_title:  Mistakes Found 

message: "The Galvanic cell, named after Luigi Galvani, consists of two metals connected by an electrolyte which forms a salt bridge between the metals. It is also known as a voltaic cell and an electrochemical cell."
1. As far as I know, the galvanic cell contains 2 electrolytes.
: Meaning that when the solutions are CuSO4 and ZnSO4, there would be both a copper electrolyte and a zinc one? As there is a copper electrode and a zinc electrode? The definition of electrolyte is not clear- here or on it's page. Loggie
2. I've never heard those two electrolytes being referred to as a salt bridge. Salt bridge is a replacement to the porous disk, the device that lets one to connect the two electrolytes without mixing.
:Yes- a salt bridge allows ions to travel from one solution to another- it is not connected/ made out of metal, as is suggested. Loggie
3. Shouldn't the voltaic, galvanic and electrochemical cell articles be merged into one?
:Are there slight differences between the three, or all they all names for the same item? Loggie
::An electrochemical cell can mean a galvanic cell, or be a general term for galvanic and electrolytic cells. Basically, a galvanic cell generates an electromotive force through a spontaneous redox reaction, where electrolysis requires an external current before the reaction will occur. splintax (talk) 07:27, 23 May 2006 (UTC)
thread_title:  Few questions 

message: You guys are just not correct in the "Description" part of the Galvanic Cell:
At the Zn anode, an atom of the the metal electrode gives up two electrons, becomes ionized ( forms a positively-charged Zn cation, Zn+2 ), and goes into the electrolyte solution, where the new cation formed is balanced by a negatively-charged sulfate anion ( SO4-2 ) coming over through the porous plate (or the salt bridge).
At the same time, at the copper cathode, a positively-charged Cu cation ( Cu+2 ) in the electrolyte solution picks up the two electrons that came over in the wire from the Zn side of the cell at the surface of the Cu metal electrode.  This converts the cation to a neutral Cu metal atom, which plates out onto the Cu electrode (Zn does NOT plate onto the copper cathode).  Since a cation disappears from the Cu+2 electrolyte solution, and a new cation appears in the Zn+2 electrolyte solution, a sulfate anion ( SO4-2 ) can cross the salt bridge to balance the change in the positive charges in the two electrolyte solutions.
The statements in the first paragraph are not true.  For every neutral Zn atom that dissolves in the ZnSO4 electrolyte, a Cu+2 cation from the CuSO4 electrolyte plates out onto the copper electrode.  The two electrons given up from the Zn side of the cell travel through the wire, do useful work, then enter the Cu electrode and convert a Cu+2 cation from the electrolyte solution to a neutral Cu atom that sticks to the Cu electrode.  At the same time, one SO4-2 anion moves through the salt bridge from the Cu side to the Zn side to balance the change in the number of cations in the two electrolyte solutions.
The picture, "Scheme Of A Galvanic Cell" should be changed: the right-pointing arrow and the words "Cation flow" should be removed.
The main point in a galvanic cell is that everything has to balance: the number of electrons given up and accepted has to be equal, the charge changes have to balance, and the anions on either side of the bridge have to balance.
Also, the number of electrons involved in the two half-reactions and the energy of those electrons (electrode potential) are two different things entirely.  The potential (EMF or voltage) has to do with the nature of the two dissimilar metals; the number of electrons transferred have to do with how many electrons the metals normally lose or gain in chemical reactions.
Starting at "In this way the anode is consumed or corroded....", the rest of the statements in the section are correct.
Also:
In the section "Electric Potential Of A Galvanic Cell", the net reaction shown isn't correct.  It should be:
            Cu+2 + Zn -> Cu + Zn+2
A suggestion:
Find a chemist to help you two write this topic. 
Old_Chemist 
68.225.187.87 10:33, 20 September 2005 (UTC)
replies: text: IIRC, both happen. Sulphate ions move to the left, and zinc ions move to the right. splintax (talk) 07:28, 23 May 2006 (UTC)
replies: text: Hmmmmm....not much of a "separator", then, is it?  ("Porous", indeed!)  So we have Alan Speigel saying zinc cations don't flow toward the cathode (to the right), and Splintax saying they do.  No wonder I'm confused! 24.6.66.193 09:40, 20 April 2007 (UTC)
thread_title:  Comments 

message: no merge
For one thing, I'm not sure that Galvonic is the correct spelling so who's going to find it there. It's an orphan, it's short, and it would fit in nicely here. Waerloeg 09:26, 25 February 2007 (UTC)
replies: text: Galvonic will die, independent of this merge discussion; but please don't move it again manually, as that detaches the page from its history. Dicklyon 04:06, 26 February 2007 (UTC)
replies: text:  But there was no significant history - and if you were mad enough to type in "galvonic corrosion" and bypass the redirect you can see what little history there was. "Galvanic corrosion" is a different page with a different history. --Wtshymanski 04:09, 26 February 2007 (UTC)
replies: text: OK, whatever; change it that way if you like, but then remove the move request, too. Dicklyon 04:18, 26 February 2007 (UTC)

text: Yes, we were both overly hasty.  Sorry.  At this point there's no longer a clear consensus, so we should wait and see. Dicklyon 05:48, 26 February 2007 (UTC)
thread_title:  Merge with [[Galvonic corrosion]] 

message: The following point was raised on the talk page for Electrolytic cell:
:A galvanic cell could also use the same metal but with different ion concentrations in solution, or maybe even with only a difference in the solution medium (ionic strength, complexing agents, etc.)
--Spoon! 11:57, 6 March 2007 (UTC)
thread_title:  not neccessarily two different metals 

message: If Zn+2 crosses the porous barrier rightwards, as was stated above, and as is indicated by the "Cation flow" arrow in the diagram, then wouldn't that cause the  solution in the right half of the cell to become contaminated with Zinc Sulfate? Does that happen in actual practice? 
If so, it would be helpful to state explicitly that it's the Zinc that disolves more quickly than the Copper in this configuration, and that it's this faster dissolution that produces the abundance of electrons at the Zinc anode, relative to the electrons produced at the more slowly dissolving Copper cathode. ( This IS correct, yes? ) When I first looked at this diagram I imagined that the Copper cathode would also (as the entry says all metals do) "become positive ions upon dissolving, and leave electrons behind", thus giving it a negative charge, just like the Zinc anode. It took me a while to figure out that even if that's so, it's the *relative* difference in the rates of electron "production" in each half-cell that gives rise to the current flow from anode to cathode. [ Edited by author on 16 March 2007 for concision only. ]64.40.60.154 15:03, 2 March 2007 (UTC)
replies: text: The copper cathode doesn't dissolve; on the contrary, it grows. --Spoon! 11:46, 6 March 2007 (UTC)
thread_title:  Clarification Request 

message: This article contains errors.  For example, the diagram is of a Daniel cell.  There may be a difference between US usage and UK usage but, in my experience, a cell for producing electricity has always been called a Voltaic cell.  Having read the articles for Alessandro Volta and Luigi Galvani I think the term Voltaic cell is much more appropriate. Biscuittin 17:29, 1 June 2007 (UTC)
thread_title:  Errors 

message: I've taken a look at the article, and made some changes. One thigh I am wondering about is, can't we merge the Corrosion and Galvanic Corrosion sections? Slapsnot (talk) 18:15, 14 May 2009 (UTC)
thread_title:  Merge Corrosion with Galvanic Corrosion 

message: the previous comment is correct.but i think we should first of all consider the reactivity of ions in the soluton with each other and with the electrodes.should the ions in the solution react with one another and with the electrodes, a salt bridge must be used. should the ions not reat with one another or react with any of the electrodes materials, a cell with a commone electrolyte may ne used. and should the ions not react with each other, but react with any of the electrode materials,a cell with a liquid junction may be used.since in this case the ions do not react with each other, but cu-2+ can react with the zn material, hence i think its advisable to use a cell with a liquid junction and not use a salt bridge. one other reason is that cells with a salt bridge are far to expensive that the other cells.  — Preceding unsigned comment added by 198.54.65.121 (talk) 07:35, 17 May 2012 (UTC)
thread_title:  on the basis of the type of galvanic 

message: I have reverted this edit which had the edit summary "tidy".  It was anything but; placing display formulae in running text makes a mess of the rendering and causes formulae on consecutive lines to overlap.  It is also deprecated for accessibility reasons.  A number of other things were changed which are largely a matter of editorial preference and therefore gratuitous.  As for moving some of the links into the See also section and then templating it for too many links is just perverse. 
Sorry for the multiple edits in the history, I was trying (unsuccessfully) to avoid having to manually redo later edits. SpinningSpark 18:08, 12 December 2012 (UTC)
thread_title:  "Tidying" edit 

message: The article makes it sound like salt bridges are the normal construction.  Aren't these just used fro educational purposes to simplify the description and/or construct an easily visible demonstration?  Has anyone actually made a practical salt bridge cell that has a real world application?  If not, I think the emphasis of the article should be changed. SpinningSpark 12:47, 28 November 2014 (UTC)
thread_title:  Salt bridge 

message: Could please somebody explain how is possible a "Galvanic cell with no cation flow" (picture on top) Isn't it that SO4(2-) anion is bigger than Zn(2+)? If so, shouldn't Zn(2+) cross the porous disk towards the copper cathode (cation flow), instead of SO4(2-) doing it in the opposite direction as described in the picture (anion flow)? Or is it another aspect than atom/molecular size that rules the ions movement through the membrane? Thank you. — Preceding unsigned comment added by Argenfox (talk • contribs) 12:08, 6 August 2019 (UTC)
thread_title:  Disk porousity  

message: Saying "Then one looks up the standard electrode potential" is incomplete.  What determines this electrode potential?  Isn't there some more fundamental principle that can be linked to or explained?  Faraday and others who first discovered this certainly could not have 'looked it up'.  — Preceding unsigned comment added by Brulez (talk • contribs) 04:27, 9 November 2020 (UTC)
replies: text: That will make the article overly detailed. A link is already provided to Standard electrode potential. --From RavenclawOIer with love 14:32, 18 February 2021 (UTC)
thread_title:  One looks up 

message: A battery includes a single cell. There is nothing improper about that. The dictionary definition cited also says "also : a single cell that furnishes electric current" so it an absurd false pedantic claim that it "properly" means more than one cell.71.63.160.210 (talk) 07:56, 10 January 2021 (UTC)
thread_title:  Incorrect Dictionary Citation 

message: I can’t edit the following sentence to clarify it, because I can’t figure out what is meant: “ The energy derives from a high-cohesive-energy metal dissolving while to a lower-energy metal is deposited, and/or from high-energy metal ions plating out while lower-energy ions go into solution.”   The odd part is “..to a lower-energy metal is deposited..”. Is something deposited to a “lower energy metal,” or is metal deposited to a lower energy unnamed thing?  Edison (talk) 17:16, 20 June 2021 (UTC)
thread_title:  Unclear sentence 

message: Full details 115.242.187.38 (talk) 04:47, 24 January 2023 (UTC)
thread_title:  Standard hydrogen electrodes