Using the enthalpy of formation (AH) given below, calculate the maximum wavelength of a light-which can dissociate NO, to NO and O. Calculate the wavelength ofa light if the reaction is to result in the complete dissociation into free atoms (i.e N + 20). [AH (kJ mol-): NO,: +33.2, NO: +90.2, N; 472.7. 0: 249 21

Using the enthalpy of formation (AH) given below, calculate the maximum wavelength of a light-which can dissociate NO, to NO and O. Calculate the wavelength ofa light if the reaction is to result in the complete dissociation into free atoms (i.e N + 20). [AH (kJ mol-): NO,: +33.2, NO: +90.2, N; 472.7. 0: 249 21

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 124CP: The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt = 1...

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The percent ionic character of the bonds in several interhalogen Molecules (as estimated from their measured dipole moments and bond lengths) are ClF (11%), BrF(15%), BrCl (5.6%), ICl(5.8%), and IBr (10%). Estimate the percent ionic characters for each of these molecules, using the equation in Problem 37, and compare them with the given values.
Determine the second ionization energy of calcium (in kJ mol-1) from the given data (all in kJ mol-1): AH°[CaCl,(s)] = -796 AH¡[Ca(g)] = 178 AH°[CI(g)] = 122 First ionization energy of Ca(g) = 590 Electron affinity of Cl(g) = -349 Lattice enthalpy of CaCl,(s) = -2260 А 1150 В 1235 C 1093 D 1210
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An important reaction in the formation of photochemicalsmog is the photodissociation of NO2:NO2 + hv---->NO(g) + O(g) The maximum wavelength of light that can cause this reactionis 420 nm. (a) In what part of the electromagnetic spectrumis light with this wavelength found? (b) What is themaximum strength of a bond, in kJ/mol, that can be brokenby absorption of a photon of 420-nm light? (c) Write out thephotodissociation reaction showing Lewis-dot structures.
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.9% Resources O Hint Consider an ionic compound, MX,, composed of generic metal M and generic gaseous halogen X. • The enthalpy of formation of MX, is AH; = -605 kJ/mol. • The enthalpy of sublimation of M is AHsub = 129 kJ/mol. • The first, second, and third ionization energies of M are IE, = 691 kJ/mol, IE2 = 1581 kJ/mol, and IE3 = 2627 kJ/mol. • The electron affinity of X is AHEA = -361 kJ/mol. (Refer to the hint). • The bond energy of X, is BE = 163 kJ/mol. Determine the lattice energy of MX3. AHjattice kJ/mol about us privacy policy terms of use contact us help careers
The average bond enthalpies of the C—F and C—Cl bondsare 485 kJ/mol and 328 kJ/mol, respectively. (a) What isthe maximum wavelength that a photon can possess andstill have sufficient energy to break the C—F and C—Clbonds, respectively? (b) Given the fact that O2, N2, andO in the upper atmosphere absorb most of the light withwavelengths shorter than 240 nm, would you expect thephotodissociation of C—F bonds to be significant in thelower atmosphere?
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