To calculate the corrosion rate of the zinc electrode, we need to determine the current flowing through the galvanic couple. We can use the Tafel equation to estimate the corrosion current density i_corr and then calculate the corrosion rate.The Tafel equation is given by:E = E_corr + b * log i/i_corr Where E is the potential 0.8 V , E_corr is the corrosion potential, b is the Tafel slope, and i is the current density.For zinc in a 0.1 M NaCl solution, the approximate values for E_corr and b are -0.76 V and 0.12 V/decade, respectively. We can rearrange the Tafel equation to solve for i_corr:i_corr = i * 10^ E - E_corr / b Assuming that the current density i is uniform across the zinc electrode surface, we can estimate i_corr:i_corr = 10^ 0.8 - -0.76 / 0.12 = 10^1.56 / 0.12 = 10^13 A/mNow, we can calculate the corrosion rate CR using Faraday's law:CR = i_corr * M * A / n * F * Where M is the molar mass of zinc 65.38 g/mol , A is the surface area of the zinc electrode 4 cm = 4 * 10^-4 m , n is the number of electrons involved in the reaction 2 for zinc , F is Faraday's constant 96485 C/mol , and is the density of zinc 7.14 g/cm .CR = 10^13 A/m * 65.38 g/mol * 4 * 10^-4 m / 2 * 96485 C/mol * 7.14 g/cm = 0.0014 cm/yearThe corrosion rate of the zinc electrode coupled to a copper electrode in a 0.1 M aqueous solution of NaCl is approximately 0.0014 cm/year.