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Water damage... causes
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<blockquote data-quote="Jay Barracato" data-source="post: 48563" data-attributes="member: 24"><p>Re: Water damage... causes</p><p></p><p>You are pulling in excessive detail that is not fully applicable. There is no way in a natural setting that you are going to have enough of a concentration difference to have a concentration cell. I was doing a thought problem based on a piece of metal placed in fairly anoxic water that does have significant ion concentration.</p><p></p><p>And I would say that kinetics does apply to equilibrium as one of the basic definitions of equilibrium is where the rates of the forward and reverse reactions are equal and that Keq can be calculated (estimated) from the rate constansts, k. At best most thermodynamic Keq are order of magnitude estimations.</p><p></p><p>I will tell you what, I will drop a piece of iron in a beaker of unagitated sea water, and we can come back in a couple of months to see what corrosion is on it.</p></blockquote><p></p>
[QUOTE="Jay Barracato, post: 48563, member: 24"] Re: Water damage... causes You are pulling in excessive detail that is not fully applicable. There is no way in a natural setting that you are going to have enough of a concentration difference to have a concentration cell. I was doing a thought problem based on a piece of metal placed in fairly anoxic water that does have significant ion concentration. And I would say that kinetics does apply to equilibrium as one of the basic definitions of equilibrium is where the rates of the forward and reverse reactions are equal and that Keq can be calculated (estimated) from the rate constansts, k. At best most thermodynamic Keq are order of magnitude estimations. I will tell you what, I will drop a piece of iron in a beaker of unagitated sea water, and we can come back in a couple of months to see what corrosion is on it. [/QUOTE]
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