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Topic: About Cu(s) + Cl(g) ---> CuCl2(s)?  (Read 21179 times)

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satha13

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About Cu(s) + Cl(g) ---> CuCl2(s)?
« on: September 20, 2005, 01:08:16 PM »
hello everybody

I am curious to know that if I bring Cu metal and let it reacts with Cl2 (g) alone. The product is CuCl2(s) right or not? But when i read about Galvanic cell in electrochemistry chapter. Cu(s) + Cl2(g) ---> CuCl2 (s) is redox reaction. It means that electron must be transferred when Cu(s) + Cl2 (g) to form CuCl2 (s) . What is the electron pathway for this reaction???? I must bring CuCl2(s) to dissolve in water first to form CuCl2 (aq). So as my understand:

Cu(s) + Cl2(g) ----> CuCl2(s) is not redox reaction because no electron movement, is it right?

Cu(s) + Cl2(g) -----> CuCl2(aq) is a redox reaction because it generates electron form Cu2+ and pass to Cl-, is it right?

I am new in chemistry, please inform me a right idea
Thank you very much :(

Offline sdekivit

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Re:About Cu(s) + Cl(g) ---> CuCl2(s)?
« Reply #1 on: September 20, 2005, 02:14:17 PM »
we start with uncharged solid Cu and the gas Cl2. In CuCl2, Cu gets the charge + 2 and hence, it loses 2 electrons. 2 Cl-atoms gain one electron because we get 2 Cl(-) in CuCl2. Now derive the so called half equation for this reaction.

(according to the table of standard electrode potentials, thgis reaction will occur:))

Offline Mitch

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Re:Can this reaction happen????
« Reply #2 on: September 22, 2005, 03:11:23 AM »
Well, calculate the delta H of the reaction and it'll give you a clue in the right direction.
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Re:Can this reaction happen????
« Reply #3 on: September 22, 2005, 04:56:58 AM »
Your question was alredy answered in General Chemistry forum.
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Re:Can this reaction happen????
« Reply #4 on: September 22, 2005, 05:43:09 AM »
Your question was alredy answered in General Chemistry forum.

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