This is not a graded question **Question**: (SHOW CALCULATIONS) If the energy of a photon is 1.27 × 10^-18 J, what is its wavelength in nm?**Answer**: To find the wavelength of a photon, we can use the relationship between energy (E), Planck's constant (h), and the speed of light (c). The equation is:\[ E = \frac{hc}{\lambda} \]where:- E is the energy of the photon.- \( h \) is Planck's constant (\( 6.626 \times 10^{-34} \) J·s).- \( c \) is the speed of light (\( 3.00 \times 10^8 \) m/s).- \(\lambda \) is the wavelength.Rearranging the equation to solve for the wavelength (\(\lambda\)):\[ \lambda = \frac{hc}{E} \]Substituting the given values:\[ \lambda = \frac{(6.626 \times 10^{-34} \text{ J·s}) \times (3.00 \times 10^8 \text{ m/s})}{1.27 \times 10^{-18} \text{ J}} \]First, calculate the numerator:\[ 6.626 \times 10^{-34} \text{ J·s} \times 3.00 \times 10^8 \text{ m/s} = 1.9878 \times 10^{-25} \text{ J·m} \]Now, divide by the energy:\[ \lambda = \frac{1.9878 \times 10^{-25} \text{ J·m}}{1.27 \times 10^{-18} \text{ J}} \approx 1.565 \times 10^{-7} \text{ m} \]Converting meters to nanometers (1 m = \(10^9\) nm):\[ \lambda = (1.565 \times 10^{-7} \text{ m}) \times (10^9 \text{ nm/m}) = 156.5 \text{ nm} \]Therefore, the wavelength of the photon is approximately 156.5 nm.

Given: The energy is 1.27 × 10-18 J. To find: Wavelength in nm

Answered: SHOW CALCULATIONS) If the energy of a…

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Chemistry

SHOW CALCULATIONS) If the energy of a photon is 1.27 x 10-18 J, what is its wavelength in nm3

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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