The pertinent reduction reaction for hard chrome plating is as follows. Cr6+ (aq
ID: 877644 • Letter: T
Question
The pertinent reduction reaction for hard chrome plating is as follows.
Cr6+ (aq) + 6 e- -----> Cr (s)
The oxidation is done through a nonsoluble electrode, so the balanced redox reaction uses 6 electrons. You want to plate a piece of steel that has a surface area of 1 ft2 = 0.093 m2. You want the thickness of the chromium layer to be 500 m.The density of chromium is 7.14 g/cm3. If the current is 50 amps, how long would the electrolysis need to be run to create the desired thickness of the hard chrome coating?
Explanation / Answer
surface area of steel = 1ft2 = 0.093 m^2
Thickness of chromium layer = 500m
density = 7.14g/cc
Volume = area*height(Thickness)
= 0.093*500 = 46.5 m^3 = 4.65*10^7 cc
mass of chromium required = Density*volume
= 4.65*10^7*7.14 = 3.32*10^8 grams
Faradays first law
w = Zit
= E/F*it
W = 3.32*10^8 grams
E = equivalent weight = gmw/charge
= 51.9961 /6 = 8.67 grams
3.32*10^8 = 8.67/96500*50*t
time = 1478108419.838 sec = 17107.736 days
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