Calculate the energy in joules per photon and kilojoules per mol for the following. energy of...
Calculate the energy in joules per photon and kilojoules per mol for the following.
energy of one photon of red light with wavelength 666.1 nm
__________________J/photon
energy of one mole photons of red light with wavelength 666.1 nm
__________________kJ/mol photon
energy of one photon of infrared radiation whose wavelength is 1256 nm
__________________J/photon
energy of one photon of infrared radiation whose wavelength is 1256 nm
__________________kJ/mol photon
energy of one photon of ultraviolet light with a frequency of 4645000000000000 Hz
__________________J/photon
energy of one photon of ultraviolet light with a frequency of 4645000000000000 Hz
__________________kJ/mol photon
Homework Answers
![le= 4645X10 Hz Ezhu = 6.626810 2 -34 Joset x 4645X10 - 1 Photon -22 T = 30,77707 x 10 ] photon LE=3077.77 x 1020 23 J . photo](http://img.homeworklib.com/questions/fcd78cf0-60a0-11eb-9d9e-9501f5b0f129.png?x-oss-process=image/resize,w_560)
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Calculate the energy in joules per photon and kilojoules per mol
for the following.
energy of...
Calculate the energy of photons, in joules per photon and kilojoules per mole, for 1000-kilocycle broadcast-band...
Calculate the energy of photons, in joules per photon and kilojoules per mole, for 1000-kilocycle broadcast-band radio waves. (one kilocycle is a frequency of a thousand hertz). What is the wavelength of such photons? How does the energy compare with that for a carbon-carbon single bond?
1. Ultraviolet radiation has a frequency of 6.8 x 101 1/3. Calculate the energy
.1. Ultraviolet radiation has a frequency of 6.8 x 101 1/3. Calculate the energy, in joules, of the photon. 2. Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 x 10101/s. 3. A sodium vapor lamp emits light photons with a wavelength of 5.89 x 10m. What is the energy of these photons? 4. One of the electron transitions in a hydrogen atom produces infrared light with a wavelength of 7.464x 10m. What amount of energy causes...
Calculate the energy per photon and the energy per mole of photons for radiation of wavelength...
Calculate the energy per photon and the energy per mole of photons for radiation of wavelength (i) 600 nm (red), (ii) 550 nm (yellow), (iii) 400 nm (blue).
A photon of light produced by a certain laser has an energy of 3.297x10-19). Calculate the...
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
calculate the wavelength and energy in joules for a single photon associated with 300 MHz signal...
calculate the wavelength and energy in joules for a single photon associated with 300 MHz signal of our new Oxford NMR. also, calculate the energy in kJ/mol for a mole of photons of this frequency.
4. Sodium lamps are commonly used to illuminate highways because of their intense yellow- orange emissions at 589 nm a. Calculate the energy, in joules, of one photon of this light. b. Calculate...
4. Sodium lamps are commonly used to illuminate highways because of their intense yellow- orange emissions at 589 nm a. Calculate the energy, in joules, of one photon of this light. b. Calculate the energy, in kilojoules, of one mole of such photons 5. What is the de Broglie wavelength (in nm) associated with a 2.5 g Ping-Pong ball traveling at 15.6 m/s? 6. What are the possible values of I and what are the possible subshells for an e...
9. Determine (a) the energy, in joules per photon, of radiation of frequency 7.39 X 1015...
9. Determine (a) the energy, in joules per photon, of radiation of frequency 7.39 X 1015 s1; (b) the mole, of radiation of energy, in kilojoules per frequency 1.97 x 1014s1.
Planck's Constant culeguatione DAX 03.00 x 10 m/s B=hxv h = 6.63 x 10" Im=1 x...
Planck's Constant culeguatione DAX 03.00 x 10 m/s B=hxv h = 6.63 x 10" Im=1 x 10nm 1 = 1000 M Wevelgem C - omet C-> 1. Ultraviolet radiation has a frequency of 6.8 * 108 1/s. Calculate the energy, in joules, of the photon. 2. Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 x 10101/s. 3. A sodium vapor lamp emits light photons with a wavelength of 5.89 x 10 m. What...
Calculate the frequency (H2), wavenumber (cm-1), energy of one photon (J/photon) and energy of one mole...
Calculate the frequency (H2), wavenumber (cm-1), energy of one photon (J/photon) and energy of one mole of photon (J/[mol of photons) of a visible light with a λ of 562 nm (10 points) 5.
The energy of light photons varies with wavelength. Calculate the energy per mole of photons for...
The energy of light photons varies with wavelength. Calculate the energy per mole of photons for each of the given colors of visible light. red light, i = 721 nm E = green light, i = 535 nm E = mol blue light, = 407 nm E = Splitting liquid water into hydrogen and oxygen requires an input of 286 kJ/mol. 286 kJ + H2O(l) — H,(g) + 0,(g) Assuming a mechanism existed in which one photon of light could...
.1. Ultraviolet radiation has a frequency of 6.8 x 101 1/3. Calculate the energy, in joules, of the photon. 2. Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 x 10101/s. 3. A sodium vapor lamp emits light photons with a wavelength of 5.89 x 10m. What is the energy of these photons? 4. One of the electron transitions in a hydrogen atom produces infrared light with a wavelength of 7.464x 10m. What amount of energy causes...
Calculate the energy per photon and the energy per mole of photons for radiation of wavelength (i) 600 nm (red), (ii) 550 nm (yellow), (iii) 400 nm (blue).
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
4. Sodium lamps are commonly used to illuminate highways because of their intense yellow- orange emissions at 589 nm a. Calculate the energy, in joules, of one photon of this light. b. Calculate the energy, in kilojoules, of one mole of such photons 5. What is the de Broglie wavelength (in nm) associated with a 2.5 g Ping-Pong ball traveling at 15.6 m/s? 6. What are the possible values of I and what are the possible subshells for an e...
9. Determine (a) the energy, in joules per photon, of radiation of frequency 7.39 X 1015 s1; (b) the mole, of radiation of energy, in kilojoules per frequency 1.97 x 1014s1.
Planck's Constant culeguatione DAX 03.00 x 10 m/s B=hxv h = 6.63 x 10" Im=1 x 10nm 1 = 1000 M Wevelgem C - omet C-> 1. Ultraviolet radiation has a frequency of 6.8 * 108 1/s. Calculate the energy, in joules, of the photon. 2. Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 x 10101/s. 3. A sodium vapor lamp emits light photons with a wavelength of 5.89 x 10 m. What...
Calculate the frequency (H2), wavenumber (cm-1), energy of one photon (J/photon) and energy of one mole of photon (J/[mol of photons) of a visible light with a λ of 562 nm (10 points) 5.
The energy of light photons varies with wavelength. Calculate the energy per mole of photons for each of the given colors of visible light. red light, i = 721 nm E = green light, i = 535 nm E = mol blue light, = 407 nm E = Splitting liquid water into hydrogen and oxygen requires an input of 286 kJ/mol. 286 kJ + H2O(l) — H,(g) + 0,(g) Assuming a mechanism existed in which one photon of light could...
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