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: Determine the energy, in joules (J), of a photon with a wavelength of 311 nm.**
**Constants:**
- Planck's constant \( h = 6.626 \times 10^{-34} \, \text{J s} \)
- Speed of light \( c = 3.00 \times 10^8 \, \text{m/s} \)
To calculate the energy of a photon, use the formula:
\[ E = \frac{h \cdot c}{\lambda} \]
Where:
- \( E \) is the energy of the photon in joules.
- \( h \) is Planck’s constant.
- \( c \) is the speed of light.
- \( \lambda \) is the wavelength in meters. (Note: Convert 311 nm to meters for calculation.)
1. Convert the wavelength from nanometers to meters:
- \( \lambda = 311 \, \text{nm} = 311 \times 10^{-9} \, \text{m} \)
2. Substitute the values into the formula and calculate \( E \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F38543b38-0ca2-4898-a226-639f5edfcbc9%2F611208ca-db1e-4796-ac1e-be35bc9cbaa8%2Fy1xbsce_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question: Determine the energy, in joules (J), of a photon with a wavelength of 311 nm.**
**Constants:**
- Planck's constant \( h = 6.626 \times 10^{-34} \, \text{J s} \)
- Speed of light \( c = 3.00 \times 10^8 \, \text{m/s} \)
To calculate the energy of a photon, use the formula:
\[ E = \frac{h \cdot c}{\lambda} \]
Where:
- \( E \) is the energy of the photon in joules.
- \( h \) is Planck’s constant.
- \( c \) is the speed of light.
- \( \lambda \) is the wavelength in meters. (Note: Convert 311 nm to meters for calculation.)
1. Convert the wavelength from nanometers to meters:
- \( \lambda = 311 \, \text{nm} = 311 \times 10^{-9} \, \text{m} \)
2. Substitute the values into the formula and calculate \( E \).
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