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Ch.14 - Chemical Kinetics
All textbooksBrown 14th EditionCh.14 - Chemical KineticsProblem 120b
Chapter 14, Problem 120b

The gas-phase reaction of NO with F2 to form NOF and F has an activation energy of Ea = 6.3 kJ/mol. and a frequency factor of A = 6.0 × 108 M-1 s-1. The reaction is believed to be bimolecular: NO(g) + F2(g) → NOF(g) + F(g) (b) Draw the Lewis structures for the NO and the NOF molecules, given that the chemical formula for NOF is misleading because the nitrogen atom is actually the central atom in the molecule.

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To draw the Lewis structure for NO, start by counting the total number of valence electrons. Nitrogen (N) has 5 valence electrons and oxygen (O) has 6 valence electrons, giving a total of 11 valence electrons for NO.
Arrange the atoms with nitrogen as the central atom and oxygen as the terminal atom. Connect them with a single bond initially, which uses 2 electrons.
Distribute the remaining 9 electrons to satisfy the octet rule, starting with the terminal atom (oxygen). Oxygen needs 8 electrons to complete its octet, so place 6 more electrons around oxygen, making a total of 8 electrons around it.
Place the remaining electron on nitrogen. Since nitrogen has 5 valence electrons, it will have a total of 6 electrons around it, including the one from the bond with oxygen. This results in a double bond between nitrogen and oxygen to satisfy the octet rule for nitrogen.
For NOF, start by counting the total number of valence electrons: nitrogen has 5, oxygen has 6, and fluorine has 7, giving a total of 18 valence electrons. Place nitrogen in the center, with oxygen and fluorine as terminal atoms. Connect nitrogen to oxygen and fluorine with single bonds initially, using 4 electrons. Distribute the remaining electrons to satisfy the octet rule for each atom, adjusting bonds as necessary.

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Open Question
Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 _x001E_C of 1.0 * 10^-5 s^-1. Calculate the partial pressure of O2 produced from 1.00 L of 0.600 M N2O5 solution at 45 _x001E_C over a period of 20.0 h if the gas is collected in a 10.0-L container. (Assume that the products do not dissolve in chloroform.)
Textbook Question

The reaction between ethyl iodide and hydroxide ion in ethanol (C2H5OH) solution, C2H5I(alc) + OH-(alc) → C2H5OH(l) + I-(alc), has an activation energy of 86.8 kJ/mol and a frequency factor of 2.10 × 1011 M-1 s-1. (c) Which reagent in the reaction is limiting, assuming the reaction proceeds to completion?

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Textbook Question

The reaction between ethyl iodide and hydroxide ion in ethanol (C2H5OH) solution, C2H5I(alc) + OH-(alc) → C2H5OH(l) + I-(alc), has an activation energy of 86.8 kJ/mol and a frequency factor of 2.10 × 1011 M-1 s-1. (d) Assuming the frequency factor and activation energy do not change as a function of temperature, calculate the rate constant for the reaction at 50 C.

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Textbook Question

The gas-phase reaction of NO with F2 to form NOF and F has an activation energy of Ea = 6.3 kJ>mol. and a frequency factor of A = 6.0 * 108 M-1 s-1. The reaction is believed to be bimolecular: NO1g2 + F21g2 ¡ NOF1g2 + F1g2 (e) Suggest a reason for the low activation energy for the reaction.

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Textbook Question

The mechanism for the oxidation of HBr by O2 to form 2 H2O and Br2 is shown in Exercise 14.74. (a) Calculate the overall standard enthalpy change for the reaction process.

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Textbook Question

The mechanism for the oxidation of HBr by O2 to form 2 H2O and Br2 is shown in Exercise 14.74. (c) Draw a plausible Lewis structure for the intermediate HOOBr. To what familiar compound of hydrogen and oxygen does it appear similar?

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