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Enter your answer in the provided box. Calculate the de Broglie wavelength (in nm) of a hydrogen atom (m =1.674 × 10-2" kg) moving at 1510 cm/s. nm

Enter your answer in the provided box. Calculate the de Broglie wavelength (in nm) of a hydrogen atom (m =1.674 × 10-2" kg) moving at 1510 cm/s. nm

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: Calculate the de Broglie Wavelength** **Problem Statement:** Calculate the de Broglie wavelength (in nm) of a hydrogen atom with a mass (\(m\)) of \(1.674 \times 10^{-27}\) kg moving at a speed of 1510 cm/s. **Instructions:** Enter your answer in the provided box. **Answer Box:** \[ \boxed{\text{ nm}} \] **Explanation:** To calculate the de Broglie wavelength, use the formula: \[ \lambda = \frac{h}{mv} \] where: - \(\lambda\) is the de Broglie wavelength, - \(h\) is the Planck constant (\(6.626 \times 10^{-34} \, \text{J s}\)), - \(m\) is the mass of the particle (\(1.674 \times 10^{-27} \, \text{kg}\)), - \(v\) is the velocity of the particle (\(1510 \, \text{cm/s} = 15.10 \, \text{m/s}\), converting cm/s to m/s). Calculate \(\lambda\) and convert the result to nanometers (1 m = \(10^9\) nm).
Transcribed Image Text:**Question: Calculate the de Broglie Wavelength** **Problem Statement:** Calculate the de Broglie wavelength (in nm) of a hydrogen atom with a mass (\(m\)) of \(1.674 \times 10^{-27}\) kg moving at a speed of 1510 cm/s. **Instructions:** Enter your answer in the provided box. **Answer Box:** \[ \boxed{\text{ nm}} \] **Explanation:** To calculate the de Broglie wavelength, use the formula: \[ \lambda = \frac{h}{mv} \] where: - \(\lambda\) is the de Broglie wavelength, - \(h\) is the Planck constant (\(6.626 \times 10^{-34} \, \text{J s}\)), - \(m\) is the mass of the particle (\(1.674 \times 10^{-27} \, \text{kg}\)), - \(v\) is the velocity of the particle (\(1510 \, \text{cm/s} = 15.10 \, \text{m/s}\), converting cm/s to m/s). Calculate \(\lambda\) and convert the result to nanometers (1 m = \(10^9\) nm).
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