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7. Dinitrogen monoxide, N2O, can decompose to nitrogen and oxygen gas: 2 N20(g) → 2 N2(g) + O2(g) Use bond dissociation enthalpies (see Table on last page) to estimate the enthalpy change for this reaction. (Hini As in problem #6, first draw the Lewis structures of the reactants and products that obey the octet rule so you kn the types of bonds involved to determine their bond dissociation energies. N20 has the following stable Lewis structure: :N=N-Ö: aur kT

7. Dinitrogen monoxide, N2O, can decompose to nitrogen and oxygen gas: 2 N20(g) → 2 N2(g) + O2(g) Use bond dissociation enthalpies (see Table on last page) to estimate the enthalpy change for this reaction. (Hini As in problem #6, first draw the Lewis structures of the reactants and products that obey the octet rule so you kn the types of bonds involved to determine their bond dissociation energies. N20 has the following stable Lewis structure: :N=N-Ö: aur kT

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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7. Dinitrogen monoxide, N20, can decompose to nitrogen and oxygen gas: 2 N20(g) → 2 N2(g) + O2(g) Use bond dissociation enthalpies (see Table on last page) to estimate the enthalpy change for this reaction. (Hint: As in problem #6, first draw the Lewis structures of the reactants and products that obey the octet rule so you know the types of bonds involved to determine their bond dissociation energies. N20 has the following stable Lewis structure: :N=N-Ö: bonds broleen 1 mol NEN 945 KJ 1 mot N-O 201 kJ 1146 kJ/mo I 45 kJ bonds formed 2 mol NEN Enthalpy Change { broken- formed 1 mol 0=0 498= 2388 KJ Imol AHn= 1146 - 2388=- Answer: -96 kJ/mol Draw the Lewis structure for the cyanide ion, CN. In aqueous solution, this ion interacts with H* to form the acid. Should the acid formula be written as HCN or CNH ? (i.e. Does the H* attach to the C or the N ?) Explain. 8. 1Ang he Pedie ech of the llewing sets f he least e 9. The formula for nitryl chloride is CINO2. A. Draw the Lewis structures for the molecule, including all resonance structures that obey the octet rule. Note tha N is the least electronegative element in the compound; hence, it would occupy the central position. plerity A hle B. What is the average N-O bond order, based on the most stable structure ?
Transcribed Image Text:7. Dinitrogen monoxide, N20, can decompose to nitrogen and oxygen gas: 2 N20(g) → 2 N2(g) + O2(g) Use bond dissociation enthalpies (see Table on last page) to estimate the enthalpy change for this reaction. (Hint: As in problem #6, first draw the Lewis structures of the reactants and products that obey the octet rule so you know the types of bonds involved to determine their bond dissociation energies. N20 has the following stable Lewis structure: :N=N-Ö: bonds broleen 1 mol NEN 945 KJ 1 mot N-O 201 kJ 1146 kJ/mo I 45 kJ bonds formed 2 mol NEN Enthalpy Change { broken- formed 1 mol 0=0 498= 2388 KJ Imol AHn= 1146 - 2388=- Answer: -96 kJ/mol Draw the Lewis structure for the cyanide ion, CN. In aqueous solution, this ion interacts with H* to form the acid. Should the acid formula be written as HCN or CNH ? (i.e. Does the H* attach to the C or the N ?) Explain. 8. 1Ang he Pedie ech of the llewing sets f he least e 9. The formula for nitryl chloride is CINO2. A. Draw the Lewis structures for the molecule, including all resonance structures that obey the octet rule. Note tha N is the least electronegative element in the compound; hence, it would occupy the central position. plerity A hle B. What is the average N-O bond order, based on the most stable structure ?
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