QUESTION 20 What is the wavelength of a photon that can just break a Nitrogen/Nitrogen Triple...
It takes 945. kJ/mol to break a nitrogen-nitrogen triple bond. Calculate the maximum wavelength of light for which a nitrogen-nitrogen triple bond could be broken by absorbing a single photon. Round your answer to 3 significant digits. xs ?
It takes 1.57 × 10-18 ) of energy to break a nitrogen-nitrogen triple bond, wavelength = 251 nm be able to break this bond? Will a photon of light with Planck's constant h = 6.63 x 10-34 Js. The speed of light c = 3.00 x 108 m/s. Yes, because the frequency of the light is low enough Yes, because the energy of the photon is high enough No, because the energy of the photon is too high No, because...
Interconverting wavelength, frequency and photon energy It takes 157 kJ/mol to break a nitrogen-oxygen single bond. Calculate the maximum wavelength of light for which a nitrogen-oxygen single bond could be broken by absorbing a single photon. Round your answer to 3 significant digits. x 5 ?
Photolysis of carbon monoxide can occur according to the following rxn: CO + hν --> C + O (delta)H = 1079 kJ/mole What wavelength of light does this correspond to in m and nm? (1079 kJ/mol) * (1000 J/1 kJ) * (1 mol/6.02*1023 photons) = 1.792 * (10^-18 J/photon) ([6.6 * 10^ -34 J/s) * (3.0*10^8 m/s)] / 1.792 * 10^-18 J/photon = 1.1 * 10^7 m or 110 nm
What is the wavelength of the photon emitted when an electron in a hydrogen atom which is in the initial state n = 8 jumps to the final state n = 2? How do you solve to get C as the correct answer? 2) What is the wavelength of the photon emitted when an electron in a hydrogen atom which is in the initial state n 8 jumps to the final staten 2? (c J 3.00 x 108 m/s, h...
A photon has an energy of 7.9 x 10-20 J. What is its wavelength? (Planck’s constant is h is 6.63 x 10-34 J s-1; the speed of light is 2.99 x 108 m sec-1).
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...
Question 17 of 20 Submit What is the energy of a mole of photons that have a wavelength of 587 nm? (n = 6.626 x 10-34 Jos and c = 3.00 x 108 m/s) (1 2 3 +/- 0 x 100 Tap here or pull up for additional resources
Question 17 of 20 Submit What is the energy of a mole of photons that have a wavelength of 683 nm? (h = 6.626 x 10-34 Jos and c = 3.00 x 108 m/s) 4 5 8 7 +/- 9 0 x 100 Tap here or pull up for additional resources
Question 3 of 9 Submit What is the energy of a mole of photons that have a wavelength of 701 nm? (n = 6.626 x 10-34 J.S and c = 3.00 x 108 m/s) 1 2 3 +/- 0 x 100 Tap here or pull up for additional resources