A galvanic cell with a measured standard cell potential of 0.27 V is constructed using two beakers connected by a salt bridge. One beaker contains a strip of gallium metal immersed in a 1 M solution of GaCl,, and the other contains a piece of nickel immersed in a 1 M solution of NiC2. The half- reactions that occur when the compartments are connected are as follows: Ni2+ * (aq) + 2e¯ → Nics) Cathode: Anode: Ga(s) → Ga* (aq) + 3e- If the potential for the oxidation of Ga to Ga is 0.55 V under standard conditions, what is the potential for the oxidation of Ni to Ni2?

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A galvanic cell with a measured standard cell potential of 0.27 V is constructed using two beakers
connected by a salt bridge. One beaker contains a strip of gallium metal immersed in a 1 M solution
of GaCl,, and the other contains a piece of nickel immersed in a 1 M solution of NiC2. The half-
reactions that occur when the compartments are connected are as follows:
Cathode:
Ni2* (ag) + 2e- → Nis)
Anode:
Gas)
Ga3* (ag) + 3e-
If the potential for the oxidation of Ga to Ga³r is 0.55 V under standard conditions, what is the potential
for the oxidation of Ni to Ni?"?
Transcribed Image Text:A galvanic cell with a measured standard cell potential of 0.27 V is constructed using two beakers connected by a salt bridge. One beaker contains a strip of gallium metal immersed in a 1 M solution of GaCl,, and the other contains a piece of nickel immersed in a 1 M solution of NiC2. The half- reactions that occur when the compartments are connected are as follows: Cathode: Ni2* (ag) + 2e- → Nis) Anode: Gas) Ga3* (ag) + 3e- If the potential for the oxidation of Ga to Ga³r is 0.55 V under standard conditions, what is the potential for the oxidation of Ni to Ni?"?
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