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Physical Chemistry
- A photoemissive material has a threshold energy, Emin = 5 1019 J. Will 300. nm radiation eject electrons from the material? Explain.arrow_forwardConsider burning ethane gas, C2H6 in oxygen (combustion) forming CO2 and water. (a) How much energy (in J) is produced in the combustion of one molecule of ethane? (b) What is the energy of a photon of ultraviolet light with a wavelength of 12.6 nm? (c) Compare your answers for (a) and (b).arrow_forwardAn FM radio station broadcasts at a frequency of 101.3 MHz. What is the wavelength, in meters and nanometers, of this radiation?arrow_forward
- The net change during photosynthesis involves CO2 and H2O forming glucose (C6H12O6) and O2. Chlorophyll absorbs light in the 600–700 nm region. (a) Write a balanced thermochemical equation for formation of 1.00 mol of glucose. (b) What is the minimum number of photons with λ = 680. nm needed to form 1.00 mol of glucose?arrow_forwardThe distance to the North Star, Polaris, is approximately 6.44 × 1018 m. (a) If Polaris were to burn out today, how many years from now would we see it disappear? (b) What time interval is required for sunlight to reach the Earth?(c) What time interval is required for a microwave signal to travel from the Earth to the Moon and back?arrow_forwardIn photoelectron spectroscopy, an electron is ejected from an atom by the collision of a UV photon with the surface of the atom. The equation describing this reaction is similar to the photoelectric effect described by Einstein: hv = ½ mv + Ei, where E; is the ionization energy of the atom. In one experiment on potassium, the kinetic energy of the ejected electron was 5.34 x 10ºJ when the UV source had a wavelength of 162 nm. Calculate the ionization energy of potassium. -19arrow_forward
- Planck's constant h = 6.6256 x 10-34 J-sec; speed of light c = 2.9979 x 108 m/s For electromagnetic radiation with a wavelength of 376.6 nm: (a) What is the frequency of the radiation (in s-')? (b) What is the energy (in J) of one photon of the radiation? (c) What is the energy (in kJ) of one mole of photons of the radiation? 1.arrow_forward(a) Calculate the energy of a single photon of light with a frequency of 6.63x10¹¹ s¹. Energy = J (b) Calculate the energy of a single photon of orange light with a wavelength of 644 nm. Energy = Jarrow_forwardlast three subpartsarrow_forward
- What is the energy of H2trapped in a zeolite, which can be modeled by a particle in a cube given nX= 10,nY= 10, nZ= 10 and LX= LY= LZ= 10−9m.arrow_forwardWhat is the wavelength λ of the photon that has been released in Part B? ΔE = −2.04×10−18 J The energy of the photon emitted by the electron is related to its wavelength by E=hcλ where λ is the wavelength in meters, 6.626×10−34 J⋅s is Planck's constant, and 3.00×108 m/s is the speed of light in a vacuum.arrow_forwardW 4. (a) A laser emits light that has a frequency of 4.69 X 10¹4 s¹. What is the energy of one photon of this radiation? V (b) If the laser emits a pulse containing 5.0 X 1017 photons of this radiation, what is the total energy of that pulse? (c) If the laser emits 1.3 X 10-2 J of energy during a pulse, how many photons are emitted?arrow_forward
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