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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_forward(a) What is the lowest possible value of the principal quantum number (n) when the angular momentum quantum number (ℓ) is 1? (b) What are the possible values of the angular momentum quantum number (ℓ) when the principal quantum number (n) is 4 and the magnetic quantum number (mℓ) is 0?arrow_forward(a) Calculate the wavelength of a photon with an energy equivalent to that of an O=O bond ( 120 kcal/mol) (b) In what region of the electromagnetic spectrum does this wavelength fall? (c) If you wanted photons with energy greater than the O=O bond, would you want longer or shorter wavelengths than that which you just calculated?arrow_forward
- In 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(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_forwardThe power output of a laser is measured by its wattage, the number of joules of energy it radiates per second (1 W = 1 J s-1). A 1.70-W argon laser produces a beam of green light with a wavelength of 514.5 nm (5.145×10-7 m).(a) Calculate the energy carried by each photon. (b) Calculate the number of photons emitted by the laser per second. a) ______ J per photon b) _______ photons per secondarrow_forward
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