ray photons with a wavelength of 2.54x10 nm Express the energy numerically in kilojoules per mole. > View Available Hint(s) Ea kJ/mol

determine The energy of a radio station with a frequency of 107.1 MHz. ( 7.10x10^26 J )

Assuming the wavelength for fluorescence is observed at 475 nm and the wavelength of the phosphorescence process occurs at 523 nm, find the energy released from 12.35 g of Calcium atoms. (Assume that there is 1 excited electron per calcium atom and every one of them relaxes via the processes above.) (Fluorescence occurs 2.45 times more frequently than phosphorescence)

An electron relaxes from the n = energy. Calculate the energy, in Joules, associated with this energy transition. If the transition is exothermic be sure to include the appropriate sign. (5.0000x10^0) energy level to the n = (2.00x10^0) Use the equation: - 2. 18x10-18 J ( -) ΔΕ - n²f n²i This is for administrative purposes only. Rydberg Constant = (2.1800x10^-18) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: х10

4) A sodium lamp emits yellow light with a wavelength of 589 nm. What is the energy, E, in kJ/mol of this light? Use h= 6.626 x 10-³4 J s c = 2.998 x 10⁰ m s-¹ N₁ = 6.022 x 1023 mol-¹

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Which one is false?

5. The human eye can detect as little as 2.5*10-¹6 joules of light. How many photons of green (510nm) light can your eye detect? How many photons of red (620nm) light can your eye detect? 6. An unknown metal sample is interrogated using a beam of X-rays to liberate electrons which are then caught by a detector that determines their kinetic energy. A beam of X-rays with wavelength 9.54nm irradiate the surface of this metal, and the detector observes electrons with kinetic energies equal to 7.3716*10 J. What is the binding energy of this unknown metal sample.