Zn(s)--- Zn2+(aq)+2e-and Ni2+(aq)+e----Ni(s)
Zn(s)--- Zn2+(aq)+2e-and Ni2+(aq)+e----Ni(s)
Ni^2+ + 2e- ===> Ni Eº = -0.25 VZn^2+ + 2e- ===> Zn Eº = -0.76 V
From the standard reduction potentials, Ni will be the cathode and Zn the anode.
Half reactions:
Zn(s) ==> Zn^2+ + 2e- anode - oxidation
Ni^2+ + 2e- ==> Ni(s) cathode - reduction
Zn2+(aq) + 2e- Zn(s) and Mg(s) Mg2+(aq) + 2e-
Zn(s) - Zn2+(aq) + 2e- and Ni2+(aq) + 2e - Ni(s)
Zn(s)-> Zn2+(aq)+2e- and Ni2+(aq) + 2e- ->Ni(s)
Zn(s)-> Zn2+(aq)+2e- and Ni2+(aq) + 2e- ->Ni(s)
Ni2+(aq) + 2e- Ni(s) and Mg(s) Mg2+(aq) + 2e-
Ni(s) | Ni2+(aq) Ag+(aq) | Ag(s)
That depends on the type of battery. There are nickel cadmium, lithium, lead acid,
Covalent bond
Ni2+(aq) + 2e- Ni(s) and Mg(s) Mg2+(aq) + 2e-
Zn(s)-> Zn2+(aq)+2e- and Ni2+(aq) + 2e- ->Ni(s)
Ni2+(aq) + 2e- Ni(s) and Mg(s) Mg2+(aq) + 2e-
Al(s) | Al3+(aq) Ni2+(aq) | Ni(s)
Answer this question… 1.05 V
Ni(s) | Ni2+(aq) Ag+(aq) | Ag(s)
Ni2+(aq) + 2e- Ni(s) and Mg(s) Mg2+(aq) + 2e-
Batteries can be classified in two waysPrimary Cell- Primary cell is a battery that is designed to be used once after that it can't be recharged with electricity examples are - AAA Cell (carbon Zinc battery) used in wall clocks,wrist watches etc.Secondary cell- Secondary cell is a battery which can be recharged multiple times with electricity such batteries are- Ni-cad battery, Li-ion battery(used in mobile phones)lead acid battery -used for Back up in homes and office etc.
No, the voltage is determined by the technology of the cell: Ni-Cad 1.2 v Alkaline 1.5 v Zinc chloride 1.6v Lithium 3 v
Al | Al^3+ Zn^2+ | Zn
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