22 - e)reduction, it gains e-ZN (s) + Cu2+ (aq)...

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Chemistry 4/22 Homework Due Thurs: 1,2,3,6,7,9,13 Batteries, aka galvanic cells a device that converts the energy released in a spontaneous reaction into electrical energy reactants actually transfer electrons flow of electrons produces electricity to power items redox reactions oxidation--loss of electrons Reduction--gain of electrons OIL RIG or LEO says GER
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soxidize reduced Cd-->Cd2+ + 2e- 2 Ni3+ + 2e- --> 2 Ni2+ 2Ni3+ + Cd --> 2 Ni2+ + Cd2+ The cadmium gives off 2 e-, resulting in a 2+ ion Two Ni3+ ions accept the two electrons and their charge goes from 3+ to 2+ electrodes reduction occurs at the cathode oxidation occurs at the anode the cathode recieves the e- the separator carries ions to maintain flow of e- the difference in electrochemical potential between the two electrodes is voltage a)reduction, it gains e- b)oxidation, it loses e- c)reduction, it gains e- d)oxidation, it loses e-
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Unformatted text preview: e)reduction, it gains e-ZN (s) + Cu2+ (aq) --> Zn 2+ (aq) + Cu(s) Zn --> Zn2+ + 2e-Cu2+ + 2e- ---> Cu the solid is not convertible back into a liquid the electrolyte is a solution that carries current (rate of electron flow, units = amps) yeppers, all the same voltage! its the same material more material, longer life! Mercury batteries had the advantage of being very small, used in watches, cameras, hearing aids toxicity and disposal concerns led to alternatives Anode = Pb Figure only shows 3 cells each cell produces 2V for a total of 12V Pb + SO4 2- --> PbSO4 + 2e-Pbo2 + 4H+ + SO42- + 2e- --> PbSO4 + 2H2O Pb + PbO2 + 2H2SO4 <-> 2 PbSO4 + 2 H2O discharging v. re-charging PBSO4 is collected in lead grinds Alternator converts PbSO4 back to Pb and PbO2 heavy, corrosive dependable (works no matter the temp long lasting (~5 yrs)...
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22 - e)reduction, it gains e-ZN (s) + Cu2+ (aq)...

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