The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. ▾ Part A ▾ 2 Submit ✓ Correct Part B Previous Answers Calculate the wavelength of the absorption lines. Separate answers by a comma. A₁. Initially, electrons are in both the ground and first excited state (n=1 and n=2). A beam of light hits the gas. This beam is a continuous spectrum of yellow/green light (from 495 nm to 590 nm) How many absorption line/s will there be in the spectra? [5] ΑΣΦ Submit 1 Request Answer ? n=4 nm n=3 n=2 n=1 4.2 eV 2.4 eV 2.0 eV O ev budod o EVE OF Color Wavelength Frequency Photon energy violet 380-450 nm 668-789 THz 2.75-3.26 V blue 450-495 nm 606-668 THz 2.50-2.75 V green 495-570 nm 526-606 THz 2.17-2.50 V yellow 570-590 nm 508-526 THz 2.10-2.17 V orange 500-620 nm 484-508 THz 2.00-2.10 V red 620-750 nm 400-484 THz 1.65-2.00 V V

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Students often get confused between Wien's displacement law and Planck's radiation law. Although both are historically related, yet they are conceptually different. Planck's law helps determine the spectrum of a blackbody, while Wien's law determines the relationship between peak wavelength and temperature.