Exposure to UVA and UVB light causes skin damage. If UVA light has a wavelength of 395 nm and UVB has a wavelength of 315 nm.
a) What is the energy of one phone of UVA and UVB light?
b) what is the energy contained in one mole of UVA and one mole of UVB photons?
c) if the average energy required to break a chemical bond is 374 KJ/mol, which light (UVA or UVB) is more likely to be able to break a chemical bond, causing damage to our skin? why?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Exposure to UVA and UVB light causes skin damage. If UVA light has a wavelength of...
One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 305 nm . (A) What is the energy of a photon of this wavelength? (B) What is the energy of a mole of these photons? (C) How many photons are in a 1.20 mJ burst of this radiation? (D) These UV photons can break chemical bonds in your skin to cause sunburn—a form of radiation damage. If the 305 nm radiation provides exactly the...
One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 300 nm . Part A What is the energy of a photon of this wavelength? E = 6.03•1019 J SubmitMy AnswersGive Up Incorrect; Try Again; 4 attempts remaining Part B What is the energy of a mole of these photons? E = J SubmitMy AnswersGive Up Part C How many photons are in a 1.10 mJ burst of this radiation? N = photons SubmitMy...
One type of sunburn occurs on exposure to UV light of wave lengthin the vicinity of 325 nm. a.) What is the energy of a photon of this wavelength? b.) What is the energy of a mole of these photons? c.) How many photons are in 1.00mJ burst of thisradiation? d.) These UV photons can break chemical bonds in you skin tocause sunburn~a form of radiation damage. If the 325 nm radiationprovides exactly the energy to break an average chemical...
There are two categories of ultraviolet light. Ultraviolet A ( UVA ) has a wavelength ranging from 320nm to 400nm . It is not so harmful to the skin and is necessary for the production of vitamin D. UVB, with a wavelength between 280nm and 320nm , is much more dangerous, because it causes skin cancerPART AFind the frequency ranges of UVA.Enter your answers separated with commas.fmin,fmax= 7.50
These UV photons can break chemical bonds in your skin to cause sunburn—a form of radiation damage. If the 320 nm radiation provides exactly the energy to break an average chemical bond in the skin, estimate the average energy of these bonds in kj/mol. Please provide a detail step of your methods. Thank you so very much!!!
One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 300 nm . a)What is the energy of a photon of this wavelength? E = 6.62×10−19 J B) What is the energy of a mole of these photons? E = C)How many photons are in a 1.10 mJburst of this radiation? N=_______ photons
One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 320 nm . They gave me three questions to this and please help me. The first is. What is the energy of one photon of this wavelength in J ? The second is. What is the energy of one mole of these photons in J ? The third is. How many photons are in a 1.00 mJ burst of this radiation in phtons ?...
The reason there is danger in exposure to high energy radiation is that the radiation can rupture chemical bonds. In some cases cancer can be caused by it. A C-C single bond has a bond energy of aprox 348 kJ/mol. What wavelength ( in nm) of light is required to provide sufficient energy to break the C-C bond?
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...
L THE ANSWER OURES 1. Quantized Energy and Photons a) Calculate the wavelength of light that has a frequency of 1.66 x 10s1 b) Calculate the wavelength of a photon that has an energy of 5.25 x 10-19 j c) A mole of yellow photons of wavelength 527 nm has kJ of energy 2. Orbitals and Quantum N