①E=hf = (6.63x1024 3.0) (6.8×105/12) = 4.5x108 5 ②E-hf = (6,63x1024 J-3) (791x100th₂) = 524x102J/ ③ 30000ml = --3 5.8915m (5.09x1014112) (663x102430) = 3.37x10-J J) 4 (3 * 10 ^ 7 - 6)/(746.4a * 0 ^ - 4 * m) =(4.02*10 4 16 (66(3*10^ -34 5)= underline 2.66*10^ -7 ) E = hf / (66210 ^ 75 * J) * (2.4 * 10 ^ 17 * 443) = boxed 1.59*0^ -25 J ) 4 1 - 39 * 10 ^ - 12 * k * 5 ⑥ 30 €6.00×104)(6.63-010733) 6 500x10m 3.98 * 10 ^ - 19 5 f= E h = (2.34 a10^ -17 5) 663*10^ -17 +1 ) =( 3.6 * 10 ^ 17 + 1/2 f= E m = (1.4 * 10 ^ - 17 * J) 663*10^ -17 JJ.) = boxed 211*10^ 2 /2 2.11 * 10 ^ (12/(1k)) C E=f-300x102= 1,42x104/cr 00001423 9434 E = 300x1024 69141014/12 (663x1025)= f-434-10 4.58-10-145 Planck's Constant Worksheet Name Date Period Max Planck explained that energy was transferred in chunks known as quanta, equal to v. The variable h is Planck's constant equal to 6.6262* 10 ^ - 34 rfloor -s and the variable v represents the frequency in 1 / S_{i} s ^ - 1 or Hz (Hertz). This equation allows the calculation of the energy of photons, given their frequency. If the wavelength is given, the energy can be determined by first using the light equation (c = v*lambda) to find the frequency, then using Planck's equation to calculate energy. Problem-Solving Strategy Known Frequency (v) E = hv Unknown Energy (E) useful equations c = v*lambda c = 3 * 10 ^ 8 * m / s E = hv Wavelength (2) v = c/lambda Frequency (v) E = hv Energy (E) h = 6.63 * 10 ^ - 34 * Jg 1nm = 1 * 10 ^ - 9 * m kJ = 1000J Energy (E) v = E/h Frequency (v) lambda = c/v Wavelength (2) Example: Light with a wavelength of 525 nm is green. Calculate the energy in joules for a green light photon. First find the frequency: v = c/lambda 3.00 x 10 m/s 525 1m v=5.71×10 5.71 x 10 Hz -Second find the energy E = hv E= (6.6262x10J-1)(5.71x10s)E3.78×10-19J/photon Use the equations above to answer the following questions. 1. Ultraviolet radiation has a frequency of 6.8 * 10 ^ 15 . Calculate the energy, in joules, of the photon. 2. Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 * 10 ^ 10 * Hz 3. A sodium vapor lamp emits light photons with a wavelength of 5.89 * 10 ^ - 7 * 1 . What is the energy of these photons? 4. One of the electron transitions in a hydrogen atom produces infrared light with a wavelength of 746.4 nm. What amount of energy causes this transition? 5. Find the energy in kJ for an x-ray photon with a frequency of 2.4 * 10 ^ 19 * s ^ - 1 6. A ruby laser produces red light that has a wavelength of 500 nm. Calculate its energy in joules. 7. What is the frequency of UV light that has an energy of 2.39 * 10 ^ - 18 * J ? 8. What is the wavelength and frequency of photons with an energy of 1.4 * 10 ^ - 21 * J 9. What is the energy of a light that has 434 nm? 10. What is the 3.42 * 10 ^ 11 * Hz ? lambda= c f = (3.0x107) (212x * 10 ^ 14) =(9.6*10^ -7 m

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