247a CHAPTER 6 The Structure of Atoms Electromagnetic Radiation and Planck\'s Eq

Question

247a CHAPTER 6 The Structure of Atoms Electromagnetic Radiation and Planck's Equation See Example 6.2.,) S. Green light has a wavelength of s.0 x 102 nm. What is (b (c he energy, in joules, of one photon of green light? What is the energy, in joules, of 1.0 mol of photons of green light? 6. Violet light has a wavelength of about 410 nm. What is 14. T its frequency? Calculate the energy of one photon of violet light. What is the energy of 1.0 mol of violet photons? Compare the energy of photons of violet light with those of red light. Which is more energetic? 7. The most prominent line in the emission spectrum of alu- minum is at 396.15 nm. What is the frequency of this line? What is the energy of one photon with this wave- length? Of 1.00 mol of these photons? 8. The most prominent line in the emission spectrum of magnesium is 285.2 nm. Other lines are found at 383.8 and 518.4 nm. In what region of the electromag- netic spectrum are these lines found? Which is the most energetic line? What is the energy of 1.00 mol of photons with the wavelength of the most energetic line? 15. 9. Place the following types of radiation in order of increas- ing energy per photon: (a) yellow light from a sodium lamp (b) x-rays from an instrument in a dentist's office c) microwaves in a microwave oven 16.

Explanation / Answer

5)
a)

Given:
lambda = 500 nm = 5.0*10^-7 m

Find energy of 1 photon first

use:
E = h*c/lambda
=(6.626*10^-34 J.s)*(3.0*10^8 m/s)/(5*10^-7 m)
= 3.976*10^-19 J
Answer: 4.0*10^-19 J

b)
This is energy of 1 photon

Energy of 1 mol = energy of 1 photon * Avogadro's number
= 3.976*10^-19*6.022*10^23 J/mol
= 2.394*10^5 J/mol
= 2.394*10^2 KJ/mol
Answer: 2.4*10^2 KJ/mol

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