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Cu+ is not stable and undergoes disproportion. E for cu+ disproportionation. (E ° cu2+/cu =0.153V , E ° cu+/cu=0.53V). (a) +0.683 V (b) -0.367 V (c) +0.3415 V (d) +0.367 V
I want th make a small correction to question Its cu2+/cu+ =0.153V i.e., cu2+ + e- ------> cu+ E0 = 0.153 V Now going into problem Cu+ solutions, tend to give a disproportion reaction: 2Cu+ ----- > Cu + Cu2+ cu+ + e- ------> cu E0 = 0.53 V so, nE0 = 0.53 V cu+ ------> cu2+ + e- E0 = - 0.153 V so, n E0 = - 0.153 V on adding above rxns we get 2Cu+ ----- > Cu + Cu2+ with E0 = +0.377 V Option is D
I want th make a small correction to question
Its cu2+/cu+ =0.153V i.e., cu2+ + e- ------> cu+ E0 = 0.153 V
Now going into problem
Cu+ solutions, tend to give a disproportion reaction: 2Cu+ ----- > Cu + Cu2+
cu+ + e- ------> cu E0 = 0.53 V so, nE0 = 0.53 V
cu+ ------> cu2+ + e- E0 = - 0.153 V so, n E0 = - 0.153 V
on adding above rxns we get 2Cu+ ----- > Cu + Cu2+ with E0 = +0.377 V
Option is D
The relationship between standard gibbs energy change for a reaction and its cell potential is ΔGo=−nFEcello. For copper electrodes, ΔGCu2+∣Cuo=ΔGCu2+∣Cu+o+ΔGCu+∣Cuo −nFECu2+∣Cuo=−nFECu2+∣Cu+o−nFECu+∣Cuo 2×ECu2+∣Cuo=1×ECu2+∣Cu+o+1×ECu+∣Cuo Substitute values in the above equation. 2×ECu2+∣Cuo=1×ECu2+∣Cu+o+1×ECu+∣Cuo =0.153V+0.53V ECu2+∣Cu=0.3415 V
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