11) OH is an important oxidant in the atmosphere. The OH bond energy is 467 kJ/mole....
Q4.18: In order to break a F-F bond, an energy of 153 kJ is required per mole of F-F bonds. What wavelength of light would be required to break a single F--F bond? Answer: nm
What is the energy (in kJ) of one mole of photons of ultraviolet light with a wavelength of 85 nm? Group of answer choices a. 1.4 × 10−6 kJ b. 2.4 ×10−15 kJ c. 2.4 × 1014 kJ d. 1.4 ×103 kJ
A carbon-iodine bond strength is listed as 241.0 kJ/mol. What energy is required to break a single C-l bond? What wavelength of light (nm) corresponds to a photon that contains enough energy to break a C-l bond? Would a C-H (443.3 kJ/mol), require a shorter or longer wavelength to be broken?
What is the energy in kJ of a mole of photons with a wavelength of 440 nm?
3. About 463 kJ/mole of energy are needed to break the H - O bond in water. Calculate the wavelength of EM energy (in nanometers) needed to break this bond. Nav = 6.022 x 1023
Calculate the wavelength (nm) and energy (kJ/mole) for an electron, in a Hydrogen atom, undergoing a transition from n = 200 to n = = 1. Type your answer in the space provided below: Enter the wavelength in nanometers and the Energy in kilojoules per mole. Wavelength (in nanometers) Energy (in kilojoules per mole) =
It takes 208.4 kJ of energy to remove 1 mole of electrons from an atom on the surface of rubidium metal. How much energy does it take to remove a single electron from an atom on the surface of solid rubidium? J What is the maximum wavelength of light capable of doing this? nm
A cobalt laser emits a beam that has 319 kj of energy per mole. What is the wavelength of this light?
Calculate the energy emitted per mole of photons (kJ/mol), by a neon sign with a frequency of 4.89 x 10" Hz. 2. A heat lamp produces 25.5 watts of power at a wavelength of 6.50 um. How many photons are emitted per second? (1 watt - 1 J/s) An electron in a hydrogen atom relaxes to the n-2 level emitting light of wavelength 410.2 nm. What is the value of n for the level where the electron originated? Hint: Use...
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...