How many electrons are being transferred in the following redox reaction?
Cu(s) + ZnCl2(aq) --> Zn(s) + CuCl2(aq)
2007-10-11 08:50:20 · 4 answers · asked by Sky N. 1 in Science & Mathematics ➔ Chemistry
Two(2)
Cu(s) = Cu^2(aq)+ + 2e-
Zn^2+(aq) + 2e- = Zn(s)
Copper loses two electrons which are gained by 'zinc'.
The 'Chloride' ion is only a 'passenger'. It neither gains nor looses electrons.
2007-10-11 09:04:36 · answer #1 · answered by lenpol7 7 · 0⤊ 0⤋
Two electrons. Cu is oxidised to Cu+2, so it loses two of its valence electrons. These two electrons are accepted by Zn+2 ions in zinc chloride solution, thus it is reduced to Zn0.
2007-10-11 08:58:05 · answer #2 · answered by wmorethaneternityw 1 · 0⤊ 0⤋
you should verify the total replace in beneficial OR damaging oxidation numbers. which would be your answer. Cr2O7(2-) + 6Cl- + 14H+ -> 2Cr3+ + 3Cl2 + 7H2O Cr adjustments from +6 to +3, so an atom of Cr selections up 3 electrons. yet there are 2 atoms of Cr, so the total replace is -6. Cl adjustments from -a million to 0, so it loses i electron. because of the fact there are 6, the total replace is +6. those numbers journey, and because they have opposite signs and indications the equation is balanced. to that end, the selection is your answer. 6 moles of electrons are transferred.
2016-12-29 05:08:41 · answer #3 · answered by liebro 3 · 0⤊ 0⤋
None. That reaction could not occur. It would have to be:
CuCl2(aq) + Zn(s) ===> Cu(s) + ZnCl2(aq)
2007-10-11 08:55:51 · answer #4 · answered by steve_geo1 7 · 0⤊ 0⤋