To calculate the corrosion rate of iron in a galvanic couple with copper, we need to determine the mass loss rate of iron due to the galvanic corrosion. The corrosion rate can be calculated using Faraday's Law of Electrolysis:Corrosion rate = i A M / n F where:- i is the current density 0.6 mA/cm - A is the area of the iron electrode 8 cm - M is the molar mass of iron 55.85 g/mol - n is the number of electrons involved in the redox reaction 2 for iron, as it forms Fe ions - F is Faraday's constant 96,485 C/mol First, we need to convert the current density from mA/cm to A/cm:0.6 mA/cm = 0.6 10 A/cm = 0.0006 A/cmNow we can calculate the corrosion rate:Corrosion rate = 0.0006 A/cm 8 cm 55.85 g/mol / 2 96,485 C/mol Corrosion rate = 0.02664 g/mol / 192,970 C/mol Corrosion rate = 1.38 10 g/CTo find the corrosion rate in terms of mass loss per unit time, we need to multiply the corrosion rate by the total current i A :Total current = 0.0006 A/cm 8 cm = 0.0048 AMass loss rate = 1.38 10 g/C 0.0048 AMass loss rate = 6.62 10 g/sThe corrosion rate of iron in the galvanic couple with copper is approximately 6.62 10 g/s.