Predicting whether a reaction will occur using standard electrode potentials
Posted: Mon Mar 06, 2023 2:36 pm
Chlorine gas is bubbled through a solution of nickel sulfate. Using standard reduction potentials, would a reaction occur?
The half reactions must begin with the reactants available: Cl[sub]2[/sub], Ni 2+ and SO[sub]4[/sub] 2- ions.
The 2 half reactions are:
Cl[sub]2[/sub] + 2e => 2Cl- Eo = +1.36 V
Ni 2+ + 2e => Ni Eo = -0.24 V
The more positive reduction potential will reduce, moving in the forward direction. Cl’s half reaction is viable because if it moves forward chlorine gas is available initially as per the scenario.
Though, the more negative reduction potential will move in the backward reaction, meaning for Ni, it starts with Ni and forms Ni 2+ ions. Since I had Ni 2+ as the only possible reactant available from the NiSO[sub]4[/sub] solution, I then concluded the reaction would not occur. The answer says that the reaction will occur and I’m unsure of which part of my reasoning is flawed.
The half reactions must begin with the reactants available: Cl[sub]2[/sub], Ni 2+ and SO[sub]4[/sub] 2- ions.
The 2 half reactions are:
Cl[sub]2[/sub] + 2e => 2Cl- Eo = +1.36 V
Ni 2+ + 2e => Ni Eo = -0.24 V
The more positive reduction potential will reduce, moving in the forward direction. Cl’s half reaction is viable because if it moves forward chlorine gas is available initially as per the scenario.
Though, the more negative reduction potential will move in the backward reaction, meaning for Ni, it starts with Ni and forms Ni 2+ ions. Since I had Ni 2+ as the only possible reactant available from the NiSO[sub]4[/sub] solution, I then concluded the reaction would not occur. The answer says that the reaction will occur and I’m unsure of which part of my reasoning is flawed.