To calculate the corrosion current density, we can use the Tafel equation, which relates the corrosion potential E_corr to the exchange current density i_0 and the corrosion current density i_corr . The Tafel equation is given by:E_corr = E_eq + b/2 * ln i_corr / i_0 where E_eq is the equilibrium potential, b is the Tafel slope usually assumed to be 120 mV/decade for the anodic and cathodic reactions , and ln is the natural logarithm. In this case, we are given E_corr -0.35 V , i_0 0.038 A/m , and we can assume b = 120 mV/decade.First, we need to convert the Tafel slope to volts/decade:b = 120 mV/decade * 1 V / 1000 mV = 0.120 V/decadeNow we can rearrange the Tafel equation to solve for i_corr:i_corr = i_0 * exp E_corr - E_eq * 2 / b Since we are not given the equilibrium potential E_eq , we can assume that the corrosion potential is close to the equilibrium potential, which means that E_corr - E_eq is small. Therefore, we can approximate i_corr as:i_corr i_0So, the corrosion current density is approximately:i_corr 0.038 A/mNext, we need to determine the corrosion rate of copper in the same environment. The corrosion rate CR can be calculated using Faraday's law:CR = i_corr * M / n * F * where M is the molar mass of copper 63.55 g/mol , n is the number of electrons involved in the corrosion reaction for copper, n = 2 , F is Faraday's constant 96,485 C/mol , and is the density of copper 8.96 g/cm .First, we need to convert the density of copper to g/m: = 8.96 g/cm * 1 m / 100 cm = 8960 g/mNow we can calculate the corrosion rate:CR = 0.038 A/m * 63.55 g/mol / 2 * 96,485 C/mol * 8960 g/m CR 6.97 10 m/yearSo, the corrosion rate of copper in 1 M HCl solution at 25C is approximately 6.97 10 m/year.