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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![**Exercise Problems on Radiation and Wavelengths**
7. **The wavelength of green light from a traffic signal is measured at 520 nm. Calculate the frequency (Convert cm to m) Note: 1 nm = \(1 \times 10^{-9}\) m.**
- **Solution approach:**
- Frequency (\(v\)) can be calculated using the formula:
\[
v = \frac{c}{\lambda}
\]
where \(c\) is the speed of light (\(3 \times 10^8\) m/s) and \(\lambda\) is the wavelength in meters.
9. **What wavelength (\(\lambda\)) of radiation has photons of energy (E) at \(2.87 \times 10^{-16}\) J? Identify the type of electromagnetic radiation.**
- **Solution approach:**
- Use the energy formula:
\[
E = \frac{hc}{\lambda}
\]
where \(h\) is Planck's constant (\(6.63 \times 10^{-34}\) Js). Rearrange to find \(\lambda\):
\[
\lambda = \frac{hc}{E}
\]
10. **A photon of visible light has a frequency (\(v\)) of \(4.3 \times 10^{14}\) s\(^{-1}\). What is the energy (E) of this photon?**
11. **Calculate the energy (E) of a photon of radiation whose wavelength (\(\lambda\)) is 322 nm.**
- **Note:** \(1 \text{ nm} = 1 \times 10^{-9} \text{ m}\).
12. **What wavelength (\(\lambda\)) of radiation has photons of energy (E) at \(2.87 \times 10^{-16}\) J?**
---
**Instructions for Solutions:**
- For frequency calculations, convert wavelength to meters before using the formula.
- For energy calculations, apply Planck’s equation rearranged for the desired variable.
- Identify the type of radiation by comparing calculated wavelength/frequency to the electromagnetic spectrum ranges.
**Note:** Detailed handwritten calculations are visible in the image, guiding through problem-solving steps, demonstrating formula applications, and providing insight into identifying electromagnetic radiation types based on context.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F58ca8a72-4839-4138-9af6-242170ab3eb7%2Fd52c5d44-e87e-40ff-a934-5fc22e520dd1%2Fgwjgvzu_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Exercise Problems on Radiation and Wavelengths**
7. **The wavelength of green light from a traffic signal is measured at 520 nm. Calculate the frequency (Convert cm to m) Note: 1 nm = \(1 \times 10^{-9}\) m.**
- **Solution approach:**
- Frequency (\(v\)) can be calculated using the formula:
\[
v = \frac{c}{\lambda}
\]
where \(c\) is the speed of light (\(3 \times 10^8\) m/s) and \(\lambda\) is the wavelength in meters.
9. **What wavelength (\(\lambda\)) of radiation has photons of energy (E) at \(2.87 \times 10^{-16}\) J? Identify the type of electromagnetic radiation.**
- **Solution approach:**
- Use the energy formula:
\[
E = \frac{hc}{\lambda}
\]
where \(h\) is Planck's constant (\(6.63 \times 10^{-34}\) Js). Rearrange to find \(\lambda\):
\[
\lambda = \frac{hc}{E}
\]
10. **A photon of visible light has a frequency (\(v\)) of \(4.3 \times 10^{14}\) s\(^{-1}\). What is the energy (E) of this photon?**
11. **Calculate the energy (E) of a photon of radiation whose wavelength (\(\lambda\)) is 322 nm.**
- **Note:** \(1 \text{ nm} = 1 \times 10^{-9} \text{ m}\).
12. **What wavelength (\(\lambda\)) of radiation has photons of energy (E) at \(2.87 \times 10^{-16}\) J?**
---
**Instructions for Solutions:**
- For frequency calculations, convert wavelength to meters before using the formula.
- For energy calculations, apply Planck’s equation rearranged for the desired variable.
- Identify the type of radiation by comparing calculated wavelength/frequency to the electromagnetic spectrum ranges.
**Note:** Detailed handwritten calculations are visible in the image, guiding through problem-solving steps, demonstrating formula applications, and providing insight into identifying electromagnetic radiation types based on context.
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