![]() ![]() If anyone could point out where I'm going wrong that would be greatly appreciated. Then subtracting the zero-point energy from $D_e$ to get $D_0$ and converting this value into kj/mol just to get an incorrect answer. Then with $\omega_e$ and $\omega_ex_e$ I used the following formula to find the dissociation energy, $D_e$, The graph below shows a best estimate of the spectrum of Hb and HbO2 from a variety. The amount of energy absorbed by the electron to. To convert from the molar extinction coefficient e to absorbance A. I feel as though my error is in this part of the problem as the question asks for a transition from v = 0 but as far as I can see in the diagram there is no peak for the v = 0 transition.įollowing this, I converted the wavelengths for each transition into wavenumbers and then subtracted the wavenumber corresponding to each transition: The dark lines, absorption lines, correspond to the frequencies of the emission spectrum of the same element. An action spectrum is a graph of the rate of biological effectiveness plotted against wavelength of light. Graph showing the effects of the Absorption Spectrum of Light. My first approach in solving this problem was selecting two transitions (v" = 2 to v' = 7 and v" = 3 to v' = 8). The action spectra of chlorophyll molecules are slightly modified in vivo depending on specific pigment-protein interactions. This phenomenon explains why wavebands, rather than a single wavelength, are absorbed. The question calls for an estimation of the energy (in kj/mol) required to dissociate ClO in its excited state when it is excited from the v = 0 of the ground state. I have been having trouble solving the following problem. Jablonski Energy Level Diagram Depicting Absorption and Fluorescence Transitions. ![]()
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