Answer:
No, because the wavelength of the light is too high.
It takes 1.57 × 10-18 ) of energy to break a nitrogen-nitrogen triple bond, wavelength =...
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 ?
QUESTION 20 What is the wavelength of a photon that can just break a Nitrogen/Nitrogen Triple bond (N=N). It takes 945 kJ to break one mole of these bonds. You can refer to the following figure to help you : EI h = 6.6 x 10-34 m2 kg/s c = 3 x 108 m/s Na = 6.02x 1023
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 ?
6. Determine the frequency (V) and energy (E) of a photon with a wavelength ) of 595 nm if E hv and v chh, where h 6.63 x 10-34 J s (Planck's constant), c 3.00 x 10+s m/s (speed of light), and 1 m 10*9 nm. Show all units and use the correct number of significant figures.
The longest wavelength of light with enough energy to break the Br–Br bond in Br2g) is 620 nm. Calculate the frequency of the light.
0. The following questions use the following value for Bond Dissociation Energy for a triple bond between two nitrogen atoms: 945kJ/mol a. Given that purple light has a wavelength of 430nm; how many purple light photons will need to completely break this triple bond? b. What is the minimum wavelength that will allow me to break that bond if I had 3.5 moles of photon? In which region of the electromagnetic spectrum will I find this light? Is this light...
When ultraviolet light with a wavelength of 400 nm falls on a certain metal surface, the maximum kinetic energy of the emitted photoelectrons is 1.10 eV .What is the maximum kinetic energy K0 of the photoelectrons when light of wavelength 310 nm falls on the same surface? Use h = 6.63×10−34 J⋅s for Planck's constant and c = 3.00×108 m/s for the speed of light and express your answer in electron volts.
Calculate Energy and Convert to Wavelength I am having problems figuring out how to solve the following problem. Show all work please. c)If the energy of a photon is 1.32 x 10 18 J, what is its wavelength in nm (c 3.00 x 108 m/s; 6.63 x 34 J. s A. 1.51 x 10-7 nm C. 1.99 x 15 nm B. 151 nm D. 1.99 x 1024 nm E. None of these choices is comect
When an electron moves from the n = 7 orbit to the n = 5 orbit of a hydrogen atom, a photon of light is emitted. What is the energy of this photon, in Joules? What is the frequency of this photon, in Hertz? What is the wavelength of this photon, in nanometers? (Eel = -2.18 x 10-18 J / n2. h = 6.63 x 10-34 Joule sec. C = 3.00 x 108 m / sec. 1 m = 1...
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).