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Cu(s) | Cu2+(aq) K+(aq) | K(s)-3.27Zn(s) | Zn2+(aq) Na+(aq) | Na(s)-1.95
0.34-(-2.37)
0.34-0.80
Zn(s) + CuSO4(aq) --> ZnSO4(aq) + Cu(s) The copper will plate out on the zinc. The net ionic reaction is: Zn(s) + Cu+2(aq) --> Zn+2(aq) + Cu(s)
For emample, if you are dealing with Copper and Zinc, you first take the half equations Cu2+ + 2e- --> Cu +0.34 Zn2+ + 2e- ---> Zn -0.76 then, you decide which one is reduced and which one is oxidized, the one with the more positive voltage is reduced, so in this case the copper is reduced. the overall reaction changes to Zn- ---> Zn2+ + 2e +0.76 Cu2+ + 2e- --> Cu +0.34 ---- Zn + Ni2+ ---> Ni + Zn2+ + 0.5 you add the voltages and get 0.5 as an experimental voltage
-2.71v
-2.71v
-2.71v
Cu(s) | Cu2+(aq) K+(aq) | K(s)-3.27Zn(s) | Zn2+(aq) Na+(aq) | Na(s)-1.95
-2.37 - 0.34
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-2.37 - 0.34
The overall voltage for a redox reaction with the half reactions Mg s -- Mg2 plus plus 2e- and Cu2 plus -- Cu is 76 V.
Lx cu 920
Cu(s)
The 5.8 Liter (352 Cu In) had around 260 to 271 h.p. and 355 lb/ft of torque. The 5.2 Liter (320 cu in) V8 had 320 h.p. Top speed was around 110 mph.
Cu(s)