3. A laser emits photons having energy of 3.74 × 10-19 J. What color would be expected for the light emitted by this laser? (c=3.00 × 10⁸ m / s, h=6.63 × 10^{-34} J · s)
a) violet
b) blue
c) green
d) yellow to orange
e) orange to red
4. What is the frequency of a photon having an energy of 9.08 × 10^{-16} J ? (c=3.00 × 10⁸ m / s, h=\right. \left.6.63 × 10^{-34} J · s)
a) 2.72 × 10^{-7} Hz
b) _______ 2.43 × 10^{-27} Hz
c) 4.11 × 10^{26} Hz
d) 1.37 × 10^{18} Hz
e) 2.19 × 10^{-10} Hz
3. A laser emits photons having energy of 3.74 x 10-19 J. What color would be expected for the light emitted...
Practice Exercise. A laser emits a pulse of light containing 3.74 x 10-16 J of energy at a frequency of 5.77 x 1013 Hz. How many photons are present in the pulse? (Answer: 9780 photons)
a. A laser emits light that has a frequency of 4.69 x 1014 s-1. What is the energy of one photon of this radiation? b. If the laser emits a pulse containing 5.0 x 1017 photons of this radiation, what is the total energy of that pulse? c. If the laser emits 1.3 x 10-2 J of energy during a pulse, how many photons are emitted?
A photon of light produced by a certain laser has an energy of 3.297x10-19). Calculate the frequency (in Hz) and wavelength (in nm) of the photon. 1 4.976e14 Hz wavelength 2 2 6025 nm What is the total energy (in kJ) in 1 mole of these photons? 198.5 xk What is the color of the emitted light? violet blue green yellow orange red
A 200-W infrared laser emits photons with a wavelength of 8.60 10-7 m, and a 200-W ultraviolet light emits photons with a wavelength of 2.64 10-7 m. (a) Which has greater energy, a single infrared photon or a single ultraviolet photon? -a single infrared photon -a single ultraviolet photon (b) What is the energy of a single infrared photon? What is the energy of a single ultraviolet photon? (c) How many infrared photons are emitted per second? How many ultraviolet...
What is the frequency of a photon having an energy of 4.91 10-17? (c-3.00 * 108 m/s, h - 6.63 x 10-34 J *S)
A laser emits light with a frequency of 1.59 Times 10^15 Hz. What is the energy of one photon of the radiation from this laser?
What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 x 10 m/s; h = 6.63 x 10-34 J·s; NA = 6.022 x 1023 moles) Select one: a. 6.46 x 10-16 J b. 6.46 x 10-25 c. 2.46 x 10-4 J Od. 12.4 kJ O e. 246 kJ
A detector absorbs 1.0 × 109 photons of monochromatic light and their total energy is found to be 0.33 nJ. What is the wavelength associated with these photons? (h = 6.63 × 10−34 J⋅s, c = 3.00 × 108 m/s) Group of answer choices 540 nm 600 nm 400 nm 500 nm
Choose the correct answer: What is the energy (E, in J) of the photons emitted by an Ar+ laser with a wavelength of l = 488 nm? a. 2.46 x 1018 J b. 2.46 x 10–18 J c. 9.69 x 10–23 J d. 4.07 x 10–19 J e. 1.36 x 10–36 J
1) A laser emits light of frequency 4.74 x 10# sec . What is the wavelength of the light in nm(l m -10 nm)? The speed of light is c 2.998 x 10* m/s. (5 pts) 2) The blue color of the sky results from the scattering of light by air molecules. The blue light has a frequency of about 7.5 x 10" Hz. (1 Hz- 1/s) a) Calculate the wavelength, in nm, associated with this radiation. 1 Hz 1s...