To calculate the corrosion rate of copper in a 0.1 M HCl solution, we can use Faraday's law of electrolysis. The formula for Faraday's law is:Corrosion rate CR = i * M * n / F * * A Where:i = current density 0.35 mA/cm M = molar mass of copper 63.546 g/mol n = number of electrons exchanged in the redox reaction 2 for copper, as Cu Cu + 2e F = Faraday's constant 96,485 C/mol = density of copper 8.96 g/cm A = area of the copper surface 1 cm First, we need to convert the current density from mA/cm to A/cm:0.35 mA/cm = 0.35 * 10^-3 A/cm = 3.5 * 10^-4 A/cmNow, we can plug in the values into the formula:CR = 3.5 * 10^-4 A/cm * 63.546 g/mol * 2 / 96,485 C/mol * 8.96 g/cm * 1 cm CR = 0.0445912 gmolC / 865.416 Cgmol CR = 5.15 * 10^-5 cm/sTo convert the corrosion rate to a more common unit, such as mils per year mpy , we can use the following conversion factor:1 cm/s = 3.170 * 10^7 mil/yearCR = 5.15 * 10^-5 cm/s * 3.170 * 10^7 mil/yearCR 1.63 mil/yearSo, the corrosion rate of copper in a 0.1 M HCl solution at 25C and atmospheric pressure with an electrode potential of -0.34 V and a current density of 0.35 mA/cm is approximately 1.63 mil/year.