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IrvPhill6636
Joined: 13 Nov 2009
Posts: 3
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 Posted: Mon Apr 26, 2010 4:48 pm Post subject: |
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Wouldn't you have to take into account that Cl- would have to be oxidized as well?
Pb + H+ + Cl- ----> Pb2+ + Cl2 + H2
Or do you just need H or Cl to make the reaction spontaneous since it completely dissociates anyways? |
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jellywing_2058
Joined: 04 May 2009
Posts: 179
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| Posted: Tue May 18, 2010 10:13 am Post subject: |
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| Quote: | Wouldn't you have to take into account that Cl- would have to be oxidized as well?
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No. To begin with, the chloride ion is a sort of spectator ion and it is ionized in an aqueous solution and will not react with itself to form chlorine gas.
Moreover, note that the reduction potential for the reduction of chlorine is much higher in comparison to either hydrogen or lead and so the reaction will not include the reduction of chlorine gas as too much energy is required. There is also no chlorine gas as a reactant to begin with.
So, the Pb(s) will reduce the H+ from HCl and release only H2(g) as correctly shown above. Cl- CANNOT be oxidized as the reduction potential is much too high and you cannot invert the reaction from Chlorine gas reduction. |
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