You decide that your chemistry professor is going down, for that test he gave yo

Question

You decide that your chemistry professor is going down, for that test he gave you! So you decide to give him a lead plated spoon (lead is not good for you). You use a battery with a current of 6.8 A, and plate a spoon in a solution of lead (IV) nitrate (PbNO3)4) for 34.5 mins. The density of lead is 11.34 g/cm3, the MW for lead = 207.2 g/mol.

What volume of lead in cm3 would have been plated on to the spoon?

The surface area of the spoon is 278.23 cm2. If you want to have a thickness of 2.56 x 10-3cm on the spoon, have you plated enough lead? Assuming the lead was plated evenly across the entire surface. Show work/ proof.

Explanation / Answer

Total charge passed = current*time in seconds = 6.8*34.5*60 = 14076 C

Thus, total equivalents of Pb electroplated = total charge/Faraday's constant = 14076/96500 = 0.146

Equivalent mass of Pb IN Pb(NO3)4 = molar mass/4 = 207.2/4 = 51.8 g/equivalent

mass of Pb deposited = equivalents*molar mass = 7.563 g

Thus, volume occupies = mass/density = 7.563/11.34 = 0.67 cm3

Now, total volume to be plated = area*thickness = 278.23*0.00256 = 0.712 cm3

Thus, not enough lead has been plated.

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