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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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The blue color of the sky results from the scattering of sunlight by air molecules. The blue light has a frequency of about 7.5 × 1014 Hz. (a) Calculate the wavelength, in nm, associated with this radiation, and (b) calculate the energy, in joules, of a single photon associated with this frequency.
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- Thermal neutrons are neutrons that move at speeds comparable to those of air molecules at room temperature. These neutrons are most effective in initiating a nuclear chain reaction among 235U isotopes. Calculate the wavelength (in nm) associated with a beam of neutrons moving at 7.00 × 102 m/s (mass of a neutron = 1.675 × 10-27 kg).arrow_forwardIf a laser emits 5.4 x 1019 photons per second and transfers a total of 87.06 J of energy over 1.93 seconds, what is the wavelength of the emitted light in nm?arrow_forwardDetermine the energy, in J, of a photon with a wavelength of 351 nm. (h = 6.626 × 10⁻³⁴ J • s and c = 3.00 × 10⁸ m/s)arrow_forward
- Ozone in the stratosphere absorbs ultraviolet light of wavelengths shorter than 320 nm, thus filtering out the most energetic radiation from sunlight. During this absorption, an ozone molecule absorbs a photon, which breaks an oxygen-oxygen bond, yielding an oxygen molecule and an oxygen atom: O3(g) + hν → O2(g) + O(g) (Here, hν denotes a photon.) Suppose a flask of ozone is irradiated with a pulse of UV light of wavelength 275 nm. Assuming that each photon of this pulse that is absorbed breaks up one ozone molecule, calculate the energy absorbed per mole of O2 produced, giving the answer in kJ/mol.arrow_forwardIf a laser emits 5.0 x 1019 photons per second and transfers a total of 80.58 J of energy over 2.06 seconds, what is the wavelength of the emitted light in nm?arrow_forwardDetermine the energy of a photon with a wavelength of 317 nm. (h = 6.626 × 10⁻³⁴ J • s and c = 3.00 × 10⁸ m/s)arrow_forward
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