**Problem Statement:**It takes 495.0 kJ of energy to remove 1 mole of electron from an atom on the surface of sodium metal. How much energy does it take to remove a single electron from an atom on the surface of solid sodium?**Questions:**1. Energy = ________ J2. What is the maximum wavelength of light capable of doing this? Wavelength = ________ nm**Options:**- Submit Answer- Try Another Version**Note:**3 item attempts remaining

Energy required to remove 1 electron=energy required to remove 1 mole of electronsNA Energy=hcλ⇒λ=hcEnergyGiven, energy required to remove 1 mole of electrons=495kJ Energy required to remove 1 electron=4956.022×1023=8.21×10-22kJ=8.21×10-19J Wavelength of light required: λ=hcE λ=6.62×10-34×3×1088.21×10-19=2.41×10-7m=241nm

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Chemistry

[References) It takes 495.0 kJ of energy to remove I mole of electron from an atom on the surface of sodium metal. How much energy does it take to remove a single electron from an atom on the surface of solid sodium? Energy = What is the maximum wavelength of light capable of doing this? Wavelength- nm

[References) It takes 495.0 kJ of energy to remove I mole of electron from an atom on the surface of sodium metal. How much energy does it take to remove a single electron from an atom on the surface of solid sodium? Energy = What is the maximum wavelength of light capable of doing this? Wavelength- nm

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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