**Hydrogen Emission Spectrum Analysis**The blue line of the hydrogen emission spectrum has a wavenumber of $ 23050 \, \text{cm}^{-1} $.**Diagram Explanation:**The image shows a segment of the hydrogen emission spectrum containing several colored lines against a black background. Each line represents a distinct wavelength of light emitted by hydrogen. Notably, one line is blue, which is the focus for this calculation.**Calculations:**1. **Calculate the Energy of One Photon of the Blue Light:** \[ \text{energy of one photon} = \underline{\hspace{3cm}} \, \text{J} \]2. **Calculate the Energy for One Mole of Photons of the Blue Light:** \[ \text{energy for one mole of photons} = \underline{\hspace{3cm}} \, \text{kJ/mol} \] These calculations require the use of the formula $ E = h \cdot c \cdot \tilde{\nu} $, where $ E $ is the energy, $ h $ is Planck's constant, $ c $ is the speed of light, and $ \tilde{\nu} $ is the wavenumber.

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tlon 3 o1 24 The blue line of the hydrogen emission spectrum has a wavenumber of 23050 cm -1 Calculate the energy of one photon of the blue light. energy of one photon = J Calculate the energy for one mole of photons of the blue light. energy for one mole of photons = kJ/mol

tlon 3 o1 24 The blue line of the hydrogen emission spectrum has a wavenumber of 23050 cm -1 Calculate the energy of one photon of the blue light. energy of one photon = J Calculate the energy for one mole of photons of the blue light. energy for one mole of photons = kJ/mol

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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