Talk:Electrochemical cell

message: I am not sure the salt bridge of the Daniell Cell is meant to let electrons move and close the circuit. As suggested in another Wikipedia's article called "Electrolyte"  electrons dont go in the electrolyte. Only ions move which means that a current would appear in the copper circuit (outside the cell)even if the circuit was open (if there wasnt resistance).
Actually, I cant find any satisfying explanation about the use of the salt bridge. Could anyone give us a hint?
From Electrolyte :
''
"When electrodes are placed in an electrolyte and a voltage is applied, the electrolyte will conduct electricity. Lone electrons normally cannot pass through the electrolyte; instead, a chemical reaction occurs at the cathode consuming electrons from the cathode, and another reaction occurs at the anode producing electrons to be taken up by the anode. As a result, a negative charge cloud develops in the electrolyte around the cathode, and a positive charge develops around the anode. The ions in the electrolyte move to neutralize these charges so that the reactions can continue and the electrons can keep flowing."
  —Preceding unsigned comment added by Whalala (talk • contribs) 09:33, 29 April 2008 (UTC)
replies: text: Yes, free electrons don't exist in water, they are far too reactive. The role of the salt bridge is to allow an electric current to pass between the two half-cells—the current is carried by the ions of the salt bridge, not by free electrons—while preventing the two electrolyte solutions from mixing. Physchim62 (talk) 11:49, 29 April 2008 (UTC)
thread_title: Salt Bridge : What's its use?

message: Do not merge.  An electrolytic cell can be very different in usage than an electrochemical cell.  As an example: electroplating is a use for an electrolytic cell, electrolytic cells are in a neutral energy state and must be driven by an external electrical force where electrochemical is an electrical source and is NOT in a neutral energy state.Jonathan888 (talk) 22:21, 11 January 2006 (UTC)
replies: text: It depends on which text you read from or which terminology you use. Some people use "electrochemical cell" to mean an electrolytic cell OR galvanic cell, but some people use it only to mean an "electrochemical cell". Maybe this should go in the article. splintax (talk) 07:23, 23 May 2006 (UTC)

text: The vote seems to be not merge.  I will remove the merge tags.--Sadi Carnot 00:52, 15 August 2006 (UTC)
thread_title: Merge debate

message: I would prefer, for several reasons, that the two not be merged.  However, if you do merge them, make sure all pages that link to Electrochemical cell will instead link to Galvanic cell, or vice versā.  This can be accomplished either by means of a redirect or by actually changing the links.  Ruff 23:52, 26 July 2006 (UTC)
replies: text: The vote seems to be not merge.  I will remove the merge tags.--Sadi Carnot 00:52, 15 August 2006 (UTC)
thread_title:  Importance of links 

message: New section to implement: types of cells
Primairy power cells are non-rechargable power cells
Secundairy power cells are rechargable power cells (also called accumulators)
This subdivision also allows a clearer view and removes the confusing "accumulator" word.
As such, perhaps accumulator-can be moved to "Secunairy power cell" and accumulator can be made a redirect.
Look into it, it makes things allot simpler.
thanks.
KVDP (talk) 13:10, 26 January 2008 (UTC)
thread_title:  Types of cells (new section) and page move to electrochemical cell to "Power cell" and accumulator to "secundairy power cell"

message: Besides NiMh (nickel-metal hydride) and NiCd (Nickel-cadmium) chemical cells, saline and  alcaline batteries (which are usually said to be 'non-rechargable cells) may also be recharged. This less-known feature allows users not only to reduce the financial expenses (saline/alcaline cells are usually cheaper) they do yearly on buying chemical cells, but also allows them to achieve environmental advantage as the batteries may be recharged up to 20 times before being exhausted (NiMh/NiCd may be recherged more however).
This recharging of saline/alcaline cells is possible trough the use of low-heat recharging (by special rechargers). Several manufacturers (as provence-piles) exist which produce these devices. Provence-piles 'Batbooster' able to recharge alcaline/saline cells Battery Xtender as another device able to recharge alcaline cells
Please include in article as this is of vital information for the environmental community. Also include my previous proposals for new sections. Also check whether using this device with NiMh/NiCd cells may increase their life expenditure aswell (so the 1000 recharges frequently mentioned may actually be achieved or surpassed).
KVDP (talk) 18:25, 2 March 2008 (UTC)
thread_title:  New section: Recharging of alcaline and saline-batteries 

message: Hi For The Cell Articlle It Says Hl Half Normal Then Half ITalic. I Need You To EXplain.  —Preceding unsigned comment added by 66.131.190.6 (talk) 22:51, 6 October 2010 (UTC)
thread_title:  CEll 

message: I originally was going to suggest that this article be merged with the Galvanic Cell article; galvanic cells should be a section of this article, since a galvanic cell is a type of electrochemical cell.  It turns out that the galvanic cell article has references and is replete with consistent information - unlike this article.  
I stop short of insisting on a merger for that reason.  This article is too poorly constructed to insist that other articles be merged into it.
In the future when people search for "Galvanic cell", assuming things are tidied up here, they will be redirected to the "galvanic cell" section of the "electrochemical cell" article.  Unfortunately, that's premature right now.  
Please voice your concerns and suggestions here.  I nearly added the merge tag to both articles, but stopped so that I could pose the idea to the community.  Spiral5800 (talk) 08:17, 12 May 2013 (UTC)
thread_title:  Merge with Galvanic Cell?  This article needs work. 

message: In the half-cell that is undergoing oxidation, the closer the equilibrium lies to the ion/atom with the more positive oxidation state the more potential this reaction will provide. Likewise, in the reduction reaction, the closer the equilibrium lies to the ion/atom with the more negative oxidation state the higher the potential.
I don't understand this sentence.
1)  ...the closer the equilibrium lies to the ion/atom with the more positive oxidation state.... How can an equilibrium lie close to an atom? Shouldn't it be some thing like "the closer the equilibrium value of  X lies to the X of the atom..." where X is some quantity like potential or concentration?
2) the higher the potential - Voltage difference? Between what and what? There is also something called electrochemical potential.  — Preceding unsigned comment added by 84.227.230.58 (talk) 10:08, 28 May 2014 (UTC)
thread_title:  Unclear 

message: In the first paragraph, it says an electro chemical cell is capable of facilitating chemical reactions through the introduction of electrical energy.  What is an example of this?  Thank you. Azulbirdyki (talk) 05:49, 25 January 2016 (UTC)
thread_title:  generation by facilitation - example?