To determine the amount of copper present in a 2-g copper wire using coulometry, we need to know the current and time required to completely dissolve the copper wire. However, since this information is not provided, we can still calculate the number of moles of copper in the wire and then relate it to the amount of charge required to dissolve it.First, we need to find the number of moles of copper in the 2-g wire. The molar mass of copper Cu is 63.55 g/mol.Number of moles = mass / molar massNumber of moles = 2 g / 63.55 g/mol = 0.0315 molNow, we need to find the amount of charge required to dissolve the copper wire. Copper has a valence of +2, meaning it requires 2 moles of electrons 2 Faradays to dissolve 1 mole of copper.Amount of charge = number of moles Faraday constant valenceAmount of charge = 0.0315 mol 96,485 C/mol 2Amount of charge = 6,078.57 CSo, 6,078.57 Coulombs of charge are required to dissolve the 2-g copper wire. However, without information on the current and time used in the coulometry experiment, we cannot provide a more specific answer to the problem.