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Determine the energy of a photon with a wavelength of 371 nm. (h = 6.626 x 10-34 J•s and c = 3.00 × 10° m/s)

Determine the energy of a photon with a wavelength of 371 nm. (h = 6.626 x 10-34 J•s and c = 3.00 × 10° m/s)

Chemistry
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 6 of 7** What is the energy of a photon with a frequency of \(7.47 \times 10^{14} \, \text{s}^{-1}\)? \((h = 6.626 \times 10^{-34} \, \text{J} \cdot \text{s})\) **Calculation Input** Below the question, there is a numeric keypad with the numbers 0-9, a clear button (C), a delete button (x), a decimal point button (.), a sign toggle button (+/-), and a scientific notation button (x 10□). Use these tools to input the energy in joules (J). **Guidance** Use the formula: \[ E = h \times f \] where \( E \) is the energy, \( h \) is Planck's constant, and \( f \) is the frequency. To find the energy: 1. Multiply Planck's constant \( 6.626 \times 10^{-34} \, \text{J} \cdot \text{s} \) by the frequency \( 7.47 \times 10^{14} \, \text{s}^{-1} \). 2. Enter the calculated result in the space provided.
Transcribed Image Text:**Question 6 of 7** What is the energy of a photon with a frequency of \(7.47 \times 10^{14} \, \text{s}^{-1}\)? \((h = 6.626 \times 10^{-34} \, \text{J} \cdot \text{s})\) **Calculation Input** Below the question, there is a numeric keypad with the numbers 0-9, a clear button (C), a delete button (x), a decimal point button (.), a sign toggle button (+/-), and a scientific notation button (x 10□). Use these tools to input the energy in joules (J). **Guidance** Use the formula: \[ E = h \times f \] where \( E \) is the energy, \( h \) is Planck's constant, and \( f \) is the frequency. To find the energy: 1. Multiply Planck's constant \( 6.626 \times 10^{-34} \, \text{J} \cdot \text{s} \) by the frequency \( 7.47 \times 10^{14} \, \text{s}^{-1} \). 2. Enter the calculated result in the space provided.
**Question 7 of 7** Determine the energy of a photon with a wavelength of 371 nm. Given: - Planck's constant (h) = 6.626 × 10⁻³⁴ J·s - Speed of light (c) = 3.00 × 10⁸ m/s --- **Instructions for Calculation:** 1. Use the formula \( E = \frac{hc}{\lambda} \) to find the energy (E) of the photon, where: - \( E \) is the energy in joules (J), - \( h \) is Planck's constant, - \( c \) is the speed of light, and - \( \lambda \) is the wavelength in meters (m). 2. Convert the wavelength from nanometers (nm) to meters: \( 371 \, \text{nm} = 371 \times 10^{-9} \, \text{m} \). **Calculator Layout:** - A numeric keypad for input. - A display labeled "J" for entering or displaying the calculated energy value. - Additional buttons include a backspace key and clear key ("C"), as well as a button for entering exponential values ("x 10"). **Note:** - Tap or pull up from the bottom to access additional resources for assistance.
Transcribed Image Text:**Question 7 of 7** Determine the energy of a photon with a wavelength of 371 nm. Given: - Planck's constant (h) = 6.626 × 10⁻³⁴ J·s - Speed of light (c) = 3.00 × 10⁸ m/s --- **Instructions for Calculation:** 1. Use the formula \( E = \frac{hc}{\lambda} \) to find the energy (E) of the photon, where: - \( E \) is the energy in joules (J), - \( h \) is Planck's constant, - \( c \) is the speed of light, and - \( \lambda \) is the wavelength in meters (m). 2. Convert the wavelength from nanometers (nm) to meters: \( 371 \, \text{nm} = 371 \times 10^{-9} \, \text{m} \). **Calculator Layout:** - A numeric keypad for input. - A display labeled "J" for entering or displaying the calculated energy value. - Additional buttons include a backspace key and clear key ("C"), as well as a button for entering exponential values ("x 10"). **Note:** - Tap or pull up from the bottom to access additional resources for assistance.
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