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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![**Question:**
What is the wavelength (in nm) of a photon if the energy is 7.17 x 10^-19 J? (h = 6.626 x 10^-34 J·s)
---
To find the wavelength (\(\lambda\)) of a photon given its energy, we can use the formula derived from Planck's equation:
\[ E = \frac{h \cdot c}{\lambda} \]
Where:
- \(E\) is the energy of the photon (7.17 x 10^-19 J),
- \(h\) is Planck's constant (6.626 x 10^-34 J·s),
- \(c\) is the speed of light (approximately \(3.00 x 10^8\) m/s),
- \(\lambda\) is the wavelength in meters.
To solve for \(\lambda\), rearrange the formula:
\[ \lambda = \frac{h \cdot c}{E} \]
Calculate \(\lambda\) and convert the result to nanometers (1 m = 10^9 nm) to get the final wavelength in nm.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2ebf2b47-0653-48b1-aa4f-9532848d4742%2F0b1f5843-102d-469f-b313-be309967505c%2Fxi8833d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
What is the wavelength (in nm) of a photon if the energy is 7.17 x 10^-19 J? (h = 6.626 x 10^-34 J·s)
---
To find the wavelength (\(\lambda\)) of a photon given its energy, we can use the formula derived from Planck's equation:
\[ E = \frac{h \cdot c}{\lambda} \]
Where:
- \(E\) is the energy of the photon (7.17 x 10^-19 J),
- \(h\) is Planck's constant (6.626 x 10^-34 J·s),
- \(c\) is the speed of light (approximately \(3.00 x 10^8\) m/s),
- \(\lambda\) is the wavelength in meters.
To solve for \(\lambda\), rearrange the formula:
\[ \lambda = \frac{h \cdot c}{E} \]
Calculate \(\lambda\) and convert the result to nanometers (1 m = 10^9 nm) to get the final wavelength in nm.
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