Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Textbook Question
Chapter 9, Problem 9.59E
Determine under what conditions of temperature and wavelength the Rayleigh-Jeans law approximates Planck’s law.
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Chapter 9 Solutions
Physical Chemistry
Ch. 9 - For an object having mass m falling in the z...Ch. 9 - For the system in exercise 9.1, determine the...Ch. 9 - Prob. 9.3ECh. 9 - Prob. 9.4ECh. 9 - Prob. 9.5ECh. 9 - List some unexplainable phenomena from the...Ch. 9 - Draw, label, and explain the functions of the...Ch. 9 - Convert a a wavelength of 218A to cm1, b a...Ch. 9 - Prob. 9.9ECh. 9 - Prob. 9.10E
Ch. 9 - Explain why no lines in the Balmer series of the...Ch. 9 - What are the series limits see the previous...Ch. 9 - The following are the numbers n2 for some of the...Ch. 9 - The Balmer series is isolated from the other...Ch. 9 - Given that the wavelengths of the first three...Ch. 9 - Some scientists study Rydberg atoms, atoms whose...Ch. 9 - Prob. 9.17ECh. 9 - Prob. 9.18ECh. 9 - a How much radiant energy is given off, in...Ch. 9 - Stefans law, equation 9.18, suggests that any body...Ch. 9 - Prob. 9.21ECh. 9 - Betelgeuse pronounced beetle juice is a reddish...Ch. 9 - An average human body has a surface area of...Ch. 9 - Prob. 9.24ECh. 9 - The slope of the plot of energy versus wavelength...Ch. 9 - a Use Wien displacement law to determine the max...Ch. 9 - Prob. 9.27ECh. 9 - Sunburn is caused by ultraviolet UV radiation. Why...Ch. 9 - Calculate the energy of photon having: a a...Ch. 9 - Prob. 9.30ECh. 9 - Integrate Plancks law equation 9.23 from the...Ch. 9 - Calculate the power of light in the wavelength...Ch. 9 - Prob. 9.33ECh. 9 - Work functions are typically given in units of...Ch. 9 - Determine the speed of an electron being emitted...Ch. 9 - Lithium has a work function of 2.90eV. Light...Ch. 9 - Prob. 9.37ECh. 9 - Assume that an electron can absorb more than one...Ch. 9 - The photoelectric effect is used today to make...Ch. 9 - Prob. 9.40ECh. 9 - Prob. 9.41ECh. 9 - Prob. 9.42ECh. 9 - Prob. 9.43ECh. 9 - Prob. 9.44ECh. 9 - Use equation 9.34 to determine the radii, in...Ch. 9 - Prob. 9.46ECh. 9 - Calculate the energies of an electron in the...Ch. 9 - Prob. 9.48ECh. 9 - Show that the collection of constants given in...Ch. 9 - Prob. 9.50ECh. 9 - Equations 9.33 and 9.34 can be combined and...Ch. 9 - a Compare equations 9.31, 9.34, and 9.41 and...Ch. 9 - Label each of the properties of an electron as a...Ch. 9 - The de Broglie equation for a particle can be...Ch. 9 - What is the wavelength of a baseball having mass...Ch. 9 - Electron microscopes operate on the fact that...Ch. 9 - Prob. 9.57ECh. 9 - Prob. 9.58ECh. 9 - Determine under what conditions of temperature and...Ch. 9 - Prob. 9.60ECh. 9 - Prob. 9.61E
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- How is the Bohr theory of the hydrogen atom inconsistent with the uncertainty principle? In fact, it was this inconsistency, along with the theorys limited application to non-hydrogen-like systems, that limited Bohrs theory.arrow_forward• use Planck’s equation to calculate the energy of a photon from its wavelength or frequency.arrow_forwardList some unexplainable phenomena from the classical science and describe what could not be explained about them at the time.arrow_forward
- 6.92 The photoelectric effect can he used to measure the value of Planck's constant. Suppose that a photoelectric effect experiment was carried out using light with v=7.501014s1 and ejected electrons were detected with a kinetic energy of 2.501011 J. The experiment was then repeated using light with v=1.001015s1 and the same metal target, and electrons were ejected with kinetic energy of 5.001011 J. Use these data to find a value for Planck’s constant. HINTS: These data are fictional and will give a result that is quite different from the real value of Planck's constant. Be sure that you do not use the real value of Planck's constant in any calculations here. It may help to start by thinking about how you would calculate the metal's binding energy if you already knew Planck's constant.arrow_forwardIn 1885, Johann Balmer, a mathematician, derived the following relation for the wavelength of lines in the visible spectrum of hydrogen =364.5 n2( n2 4) where in nanometers and n is an integer that can be 3, 4, 5, . . . Show that this relation follows from the Bohr equation and the equation using the Rydberg constant. Note that in the Balmer series, the electron is returning to the n=2 level.arrow_forwardConsider a one-dimensional particle-in-a-box and a three-dimensional particle-in-a-box that have the same dimensions. a What is the ratio of the energies of a particle having the lowest possible quantum numbers in both boxes? b Does this ratio stay the same if the quantum numbers are not the lowest possible values?arrow_forward
- Determine the speed of an electron being emitted by rubidium (=2.16eV) when light of the following wavelengths is shined on the metal in vacuum: a550nm, b450nm,c350nm.arrow_forwardVerify the specific value of a, the Bohr radius, by using the values of the various constants and evaluating equation 11.68.arrow_forwardWhat experimental evidence supports the quantum theory of light? Explain the wave-particle duality of all matter .. For what size particles must one consider both the wave and the particle properties?arrow_forward
- Some scientists study Rydberg atoms, atoms whose electron has a large value of the n quantum number. Some Rydberg hydrogen atoms may have consequences in interstellar chemistry. Predict the radius of a Rydberg hydrogen atom that has n=100.arrow_forwardImagine a world in which the rule for the l quantum number is that values start with 1 and go up to n. The rules for the n and mi quantum numbers are unchanged from those of our world. Write the quantum numbers for the first two shells (i.e., n = 1 and n = 2).arrow_forwarda For a pendulum having classical frequency of 1.00s1, what is the energy difference in J between quantized energy levels? b Calculate the wavelength of light that must be absorbed in order for the pendulum to go from one level to another. c Can you determine in what region of the electromagnetic spectrum such a wavelength belongs? d Comment on your results for parts a and b based on your knowledge of the state of science in early twentieth century. Why wasnt the quantum mechanical behavior of nature noticed?arrow_forward
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