(a) Calculate the energy of a single photon of light with a frequency of 3.00×1024 s. Energy = J (b) Calculate the energy of a single photon of yellow light with a wavelength of 575 nm. Energy = Submit Show Approach Show Tutor Steps
(a) Calculate the energy of a single photon of light with a frequency of 3.00×1024 s. Energy = J (b) Calculate the energy of a single photon of yellow light with a wavelength of 575 nm. Energy = Submit Show Approach Show Tutor Steps
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
![### Photon Energy Calculation
#### Problem (a)
Calculate the energy of a single photon of light with a frequency of \(3.00 \times 10^{24} \, \text{s}^{-1}\).
- **Energy =** \_\_\_\_\_\_ J
#### Problem (b)
Calculate the energy of a single photon of yellow light with a wavelength of \(575 \, \text{nm}\).
- **Energy =** \_\_\_\_\_\_ J
---
### Explanation
In these exercises, you are required to calculate the energy of photons. The energy of a photon can be calculated using the following formulas:
1. **Using Frequency:**
\[
E = h \cdot f
\]
Where \(E\) is the energy in joules, \(h\) is Planck's constant (\(6.626 \times 10^{-34} \, \text{J s}\)), and \(f\) is the frequency in s\(^{-1}\).
2. **Using Wavelength:**
\[
E = \frac{h \cdot c}{\lambda}
\]
Where \(\lambda\) is the wavelength in meters and \(c\) is the speed of light (\(3.00 \times 10^8 \, \text{m/s}\)). To use this formula, ensure wavelength \(\lambda\) is converted from nanometers to meters. (1 nm = \(1 \times 10^{-9}\) meters)
Approach each calculation by substituting the given values into the appropriate formula.
Below each question, you have space to enter your calculated value for the photon's energy in joules.
Useful links:
- [Submit your answer]
- [Show Approach]
- [Show Tutor Steps]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff992f4e2-01e7-4c5a-8b12-5a1f40811dcf%2F91703248-6f11-408d-990f-7cfa36bfda35%2Fy3npt6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Photon Energy Calculation
#### Problem (a)
Calculate the energy of a single photon of light with a frequency of \(3.00 \times 10^{24} \, \text{s}^{-1}\).
- **Energy =** \_\_\_\_\_\_ J
#### Problem (b)
Calculate the energy of a single photon of yellow light with a wavelength of \(575 \, \text{nm}\).
- **Energy =** \_\_\_\_\_\_ J
---
### Explanation
In these exercises, you are required to calculate the energy of photons. The energy of a photon can be calculated using the following formulas:
1. **Using Frequency:**
\[
E = h \cdot f
\]
Where \(E\) is the energy in joules, \(h\) is Planck's constant (\(6.626 \times 10^{-34} \, \text{J s}\)), and \(f\) is the frequency in s\(^{-1}\).
2. **Using Wavelength:**
\[
E = \frac{h \cdot c}{\lambda}
\]
Where \(\lambda\) is the wavelength in meters and \(c\) is the speed of light (\(3.00 \times 10^8 \, \text{m/s}\)). To use this formula, ensure wavelength \(\lambda\) is converted from nanometers to meters. (1 nm = \(1 \times 10^{-9}\) meters)
Approach each calculation by substituting the given values into the appropriate formula.
Below each question, you have space to enter your calculated value for the photon's energy in joules.
Useful links:
- [Submit your answer]
- [Show Approach]
- [Show Tutor Steps]
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