# C if you wanted to design a battery from relatively

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C.) If you wanted to design a battery from relatively common materials that produced a voltage of about 1 V which cell reaction would you choose?
D.) Why were the measurements on Mg (s) and Al (s) so difficult?
E.) The “Zebra” cell was invented in 1985 in South Africa as part of the “ZEolite Battery Research Africa” project, and is used in all-electric municipal buses and other vehicles. It
uses nickel and molten sodium as its electrodes. Its overall cell reaction is NiCl2(l) + 2Na(l) <--> Ni(s) + 2NaCl(l)1.) What is the E°for the Zebra cell?[2].
2.) Are the reactants in this battery at room temperature when it is operating? Explain how you know.
F.) Concrete used in road construction is reinforced using steel bars in a grid, known collectively as “rebar.” After many years, rebar will begin to corrode, and the concrete will weaken. Studies are ongoing regarding the best metal to be a sacrificial anode to prevent corrosion of the rebar. Which would work better for the purpose, magnesium or zinc? Explain your answer based on the oxidation potentials for each metal.
G.) How many grams of copper can be reduced (plated out) by applying a 4.00 amp current for 53.0 minutes to a solution containing Cu2+ ions?
Calculations: E.)cell= E°ox+ E°redcell= -908 mV= -0.908 Vcell- red= E°ox (-0.908 V) – (0.34 V) = -1.25 VF.)log10K = ( nE°cell) / (0.0592) log10K = (2)(0.908 V) / (0.0592)log10K = 30.67 K= e30.67K= 2.088 x 1013C.) cell= E°cathode- E°Anode1.18 V= 0.415 V- (-0.765 V) G.) Half reaction: Cu2++ 2e-Cu(s) (53.0 min) x (60 sec / 1 min) = 3180 sec(4.00 A x 3180 sec x 63.546 g/mol Cu) / (96500 C x 2 e-) = 808305.12/193000 = 4.1881 gSources:[1]. "Standard Oxidation Potentials."Standard Oxidation Potentials. N.p., n.d. Web. 29 July 2014. <>.[2]. "Standard Electrode Potentials in Aqueous Solution at 25°C."Table of Standard Electrode Potentials. N.p.,n.d. Web. 29 July 2014. <>.