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- Calculate the time, in minutes, needed to plate 17.697 g of metal M at 43 Amps. The molar mass of metal M is 57.915 g/mol. M6+ + 6 e– → M Recall that, C = A*s, and Faraday’s constant, F, is 96,485 C/mole of electrons.Which wire color is the anode?What does this phase diagram say about using Aluminum current collectors in Li metal plating and stripping cell, at room condition?
- In the video "Sacrificial Anode Materials Demo", which among Zn, Al, Mg served as as i) sacrificial anodes? and ii) as noble coatings?Tin coated steel can corrode faster than uncoated steel cans. By maling used of standard reduction potentials and half ractions explain why this is the case.A steel sheet will have a thin layer of zinc put on one side to protect it from corrosion. Determination of the zinc film thickness per one centimeter square of steel sheet when a 2 A current is employed and the electrolytic deposition process is completed in exactly 30 minutes at 25 degrees Celsius. With a 1 M zinc solution, it's safe to presume that its concentration will remain stable throughout the process.
- A cylindrical sample of solid germanium has length 55.0 mm and diameter 5.0 mm. In a test circuit, 0.150 A of current flowed through this sample when the voltage applied between its ends was 17.5 V. What is the electricalconductivity of this sample?The time needed to plate out 1.75 g Ni(Ni2+) using a 15-amp current is about 380 minutes 190 minutes 3.2 minutes 6.4 minutesThe _____ in a _____ voltammogram is related to the ____ a. limiting current, cyclic, concentration of the analyte of interest b. limiting current , linear sweep, concentration of the analyte of interest c. peak current cyclic, standard reduction potential of the analyte of interest d. peak current , linear sweep, standard reduction potential of the analyte of interest e. none of these