1. The energy needed to dissociate an oxygen molecule into oxygenatoms (the bond energy) is 498 k,J / mol. What is the maximumwavelength of light that will initiate the split of oxygenmolecule? Is visible light capable to complete thisprocess?<?xml:namespace prefix = o ns ="urn:schemas-microsoft-com:office:office" />
2.In the potassium emission spectrum quite intense line isobserved at 766.0 nm. Calculate the frequency of radiationproducing this line. Is this line visible to the eye? If yourprevious answer is yes, what is the color of this line? If not, isit at higher or lower energy than visible light? (c = 2.998x 108m/s; R = 3.2881 x 10151/s)
3. Find the energy change when an electron moves from the n = 4level to the
n = 2 level in thehydrogen atom. If this energy is emitted as a photon, what is thewavelength of this photon? (c = 2.998 x 108m/s; R = 3.2881x 10151/s)
Type your question here
1. The energy needed to dissociate an oxygen molecule into oxygenatoms (the bond energy) is 498 k,J / mol. What is the maximumwavelength of light that will initiate the split of oxygenmolecule? Is visible light capable to complete thisprocess?<?xml:namespace prefix = o ns ="urn:schemas-microsoft-com:office:office" />
2.In the potassium emission spectrum quite intense line isobserved at 766.0 nm. Calculate the frequency of radiationproducing this line. Is this line visible to the eye? If yourprevious answer is yes, what is the color of this line? If not, isit at higher or lower energy than visible light? (c = 2.998x 108m/s; R = 3.2881 x 10151/s)
3. Find the energy change when an electron moves from the n = 4level to the
n = 2 level in thehydrogen atom. If this energy is emitted as a photon, what is thewavelength of this photon? (c = 2.998 x 108m/s; R = 3.2881x 10151/s)
Type your question here
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