a. the first ionization energy of aluminum is 578 kJ/mol. How much energy is required to ionize one atom of Al? I put E= 578 kJ/mol . is this how to start? b. Write out balanced chemical equation that represents the first ionization of aluminum (you must include the physical states) c. Calculate the wavelength of a photon that has just enough energy to ionize a single atom of aluminum. d. how many moles of photons with the wavelength you calculated in part c are required to ionize 1.15 moles of aluminum? Can you help me set these up. I am studying for a test and we have not been over all of these yet? Thanks.