Given reduction potentials, like ag+(aq) + e- --> ag(s) and ni2+(aq) + 2e- -->ni(s)
In an electrochemical cell which uses nickel (Ni) and silver (Ag), which metal will be oxidized? Ni or Ag?
i think its nickel but not sure, please help!
for an electrochemical cell which uses silver (Ag) and lead (Pb), will ag be reduced?
Look up the oxidation potential of Ag and Ni (they will be the negative of the reduction potential).The one with the higher oxidation potential will be oxidized and the other will be reduced.
Do the same for Pb and Ag.
It's been awhile since I've looked at an activity series table but I believe you will find Ni to oxidize Ag ion and Pb to oxidize Ag ion but you should confirm that..
To determine which metal will be oxidized in an electrochemical cell, you can compare the reduction potentials of the metals. In the given reduction potentials, Ag+ (aq) + e- → Ag (s) has a reduction potential and Ni2+ (aq) + 2e- → Ni (s) also has reduction potential.
The general rule to determine which metal will be oxidized is that the metal with a lower reduction potential will be oxidized. In other words, the metal with the more negative reduction potential is more likely to undergo oxidation.
Comparing the reduction potentials, Ni2+ (aq) + 2e- → Ni (s) has a more negative reduction potential than Ag+ (aq) + e- → Ag (s). Therefore, nickel (Ni) will be oxidized while silver (Ag) will be reduced in this electrochemical cell.