Question: please help 6. Is normal light (visible photon energy) sufficient to break chemical bonds? Let's calculate... From the earlier table, we see that an I-I

please help please help 6. Is normal light (visible photon energy) sufficient to break

6. Is normal light (visible photon energy) sufficient to break chemical bonds? Let's calculate... From the earlier table, we see that an I-I bond (one of the weakest) has a bond energy of 151kJ/mol. In other words, it takes 151kJ of energy to break a mole of I-I bonds. How many bonds is this? (What's a mole)? How much energy (in J) would it take to break just one I-I bond? If you were providing that energy in the form of a single photon, what would its frequency have to be? (see info below). What type of photon is this? On the spectrum below, shade or identify the regions where photons might have enough energy to break covalent bonds. E=hvv=ch=6.6261034Jsecc=3.0108m/sec

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