1st Edition

ISBN: 9781307092097

Author: Chang

Publisher: MCG/CREATE

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Chapter 14, Problem 14.67QP

The equilibrium constant (K_P) for the formation of the air pollutant nitric oxide (NO) in an automobile engine at 530°C is 2.9 × 10⁻¹¹:

N 2 ( g ) + O 2 ( g ) ⇌ 2 NO ( g )

(a) Calculate the partial pressure of NO under these conditions if the partial pressures of nitrogen and oxygen are 3.0 atm and 0.012 atm, respectively. (b) Repeat the calculation for atmospheric conditions where the partial pressures of nitrogen and oxygen are 0.78 atm and 0.21 atm and the temperature is 25°C. (The K_P for the reaction is 4.0 × 10⁻³¹ at this temperature.) (c) Is the formation of NO endothermic or exothermic? (d) What natural phenomenon promotes the formation of NO? Why?

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Chapter 14, Problem 14.66QP

Chapter 14, Problem 14.68QP

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Chapter 14 Solutions

CHEMISTRY 1111 LAB MANUAL >C<

Ch. 14.1 - Consider the equilibrium XY, where the forward...Ch. 14.2 - Write Kc and Kp for the decomposition of...Ch. 14.2 - Carbonyl chloride (COCl2), also called phosgene,...Ch. 14.2 - Prob. 4PE Ch. 14.2 - Write equilibrium constant expressions for Kc and...Ch. 14.2 - Consider the following equilibrium at 395 K:...Ch. 14.2 - For which of the following reactions is Kc equal...Ch. 14.2 - You are given the equilibrium constant for the...Ch. 14.2 - Prob. 7PE Ch. 14.2 - From the following equilibrium constant...

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