Wavelength (nm)I'm not sure what equation I can come up with other than the one generated with my graph. Can youplease show me the calculations that were used to find this equation?Give an equation that relates energy to wavelength. Explain how you arrived at your equation.Wavelength Energy (kJ/mol)(nm)350341.8420284.8470254.5530225.7580206.3620192.9700170.9750159.5Energy vs. Wavelength (Graph 1)400350y=-0.4367x+470.8230025020015010050O0100200300400500600700800Energy (kJ/mol)

Answered: Wavelength (nm) I'm not sure what…

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter6: The Structure Of Atoms

Section6.2: Quantization: Planck, Einstein, Energy, And Photons

Problem 1RC

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6.101 Laser welding is a technique in which a tightly focused laser beam is used to deposit enough energy to weld metal parts together. Because the entire process can be automated, it is commonly used in many large-scale industries, including the manufacture of automobiles. In order to achieve the desired weld quality, the steel parts being joined must absorb energy at a rate of about 104 W/mm2. (Recall that 1 W = 1 J/s.) A particular laser welding system employs a Nd:YAG laser operating at a wavelength of 1.06m ; at this wavelength steel will absorb about 80% of the incident photons. If the laser beam is focused to illuminate a circular spot with a diameter of 0.02 inch, what is the minimum power (in watts) that the laser must emit to reach the 104 W/mm2 threshold? How many photons per second does this correspond to? (For simplicity, assume that the energy from the laser does not penetrate into the metal to any significant depth.)
Investigating Energy Levels Consider the hypothetical atom X that has one electron like the H atom but has different energy levels. The energies of an electron in an X atom are described by the equation E=RHn3 where RH is the same as for hydrogen (2.179 1018 J). Answer the following questions, without calculating energy values. a How would the ground-state energy levels of X and H compare? b Would the energy of an electron in the n = 2 level of H be higher or lower than that of an electron in the n = 2 level of X? Explain your answer. c How do the spacings of the energy levels of X and H compare? d Which would involve the emission of a higher frequency of light, the transition of an electron in an H atom from the n = 5 to the n = 3 level or a similar transition in an X atom? e Which atom, X or H, would require more energy to completely remove its electron? f A photon corresponding to a particular frequency of blue light produces a transition from the n = 2 to the n = 5 level of a hydrogen atom. Could this photon produce the same transition (n = 12 to n = 5) in an atom of X? Explain.
Are mathematical expressions for the following potential energies positive or negative? Explain why in each case. a The attraction between an electron and a helium nucleus b The repulsion between two protons in a nucleus c The attraction between a north and a south magnetic pole d The force of gravity between the Sun and Earth e A rock perched on the edge of a cliff with respect to the base of the cliff
When a hydrogen atom absorbs a photon of electromagnetic radiation (EMR), the internal energy of the atom increases and one or more electrons may be energized into an excited state. The release of this extra energy as the excited state electron transitions back to a lower energy state results in the emission of a photon. These energy changes are responsible for the emission spectrum of hydrogen (shown below) and are described by the Bohr equation. delta?=−2.178×10−18 J(1?2final−1?2initial)ΔE=−2.178×10−18 J(1nfinal2−1ninitial2) *refer to attached image before proceeding* To ionize a hydrogen atom (forming a hydrogen ion), requires that the energy absorbed is sufficient to send the energized electron an infinite distance away from the nucleus (as shown by the ionization line in the image above). In other words, nfinal is equal to infinity. Calculate the energy required to ionize a ground state hydrogen atom. Report your answer in kilojoules. delta E= ____kJ What is the longest…
Light in the infrared portion of the electromagnetic spectrum excites vibrations of certain molecules, causing them to move more rapidly. In this manner, infrared light can be used to heat a substance. If a 1000.-mW, 808-nm laser is used to heat a 50.0-mL sample of water from 22.0 o C to its boiling point, a) how many photons will the water absorb and b) what is the minimum amount of time this will take?
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* 00 In his explanation of the threshold frequency in the photoelectric field, Einstein reasoned that the absorbed photon must have the minimum energy required to dislodge an electron from the metal surface. This energy is called the work function (9) of that metal. What is the longest wavelength of radiation (in nm) that could cause the photoelectric effect in W, where o = 4,41 × 10 19 J? IIO 24 4 # 2 3. 9. 7.
need help with this chemistry
A local fm station broadcasts at a frequency of 702 kHz. Calculate the energy of the frequency at which it is broadcasting. Energy=??? kJ photon
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It takes 155. kJ/mol to break a fluorine-fluorine single bond. Calculate the maximum wavelength of light for which a fluorine-fluorine single bond could be broken by absorbing a single photon. Round your answer to 3 significant digits. nm |0- 0 x10 X
||| = y google - Yahoo Search Results O ELECTRONIC STRUCTURE AND CHEMICAL BONDING Understanding the organization of the electromagnetic spectrum Try Again Your answer is incorrect. • order of frequency: Your answer is incorrect. order of wavelength: Your answer is incorrect. order of energy: Your answer is incorrect. • type of radiation green light A few different types of electromagnetic radiation are listed in the table below. Complete the table by ordering these types of radiation by increasing frequency, wavelength, and energy per photon. For example, select "1" in the second column for the type of radiation with the lowest frequency, "2" for the type of radiation with the next higher frequency, and so forth. infrared radiation radio waves microwaves Explanation order of frequency (Choose one) ▼ (Choose one) (Choose one) ▼ (Choose one) ▼ pearson login - Yahoo Search Results Yahoo Search Results Recheck order of wavelength (Choose one) ▼ (Choose one) ▼ (Choose one) ▼ (Choose one)…

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