Nitrosyl chloride decomposes significantly only at elevated temperatures. At the room temperature, its decomposition is characterized by a small value of equilibrium constant: 2NOCl(g) ⇄ 2NO(g) + Cl2(g), Kp = 7.0 \times 10-8 atm at 250C Suppose you fill a container with 1.00 atm of pure NOCl (g) at 25℃ and wait until the decomposition equilibrium is established. What equilibrium partial pressures of NOCl(g), NO(g), and Cl2(g) are expected?
Nitrosyl chloride decomposes significantly only at elevated temperatures. At the room temperature, its decomposition is characterized by a small value of equilibrium constant: 2NOCl(g) ⇄ 2NO(g) + Cl2(g), Kp = 7.0 \times 10-8 atm at 250C Suppose you fill a container with 1.00 atm of pure NOCl (g) at 25℃ and wait until the decomposition equilibrium is established. What equilibrium partial pressures of NOCl(g), NO(g), and Cl2(g) are expected?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Nitrosyl chloride decomposes significantly only at elevated temperatures. At the room temperature, its decomposition is characterized by a small value of equilibrium constant: 2NOCl(g) ⇄ 2NO(g) + Cl2(g), Kp = 7.0 \times 10-8 atm at 250C Suppose you fill a container with 1.00 atm of pure NOCl (g) at 25℃ and wait until the decomposition equilibrium is established. What equilibrium partial pressures of NOCl(g), NO(g), and Cl2(g) are expected?
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