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Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl₂, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl₂(g) = 2 NOCI(g)

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl₂, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl₂(g) = 2 NOCI(g)

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 54QAP: Consider the following hypothetical reaction: X2(g)+R(s)X2R(g) R has a molar mass of 73 g/mol. When...
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Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl₂(g) = 2 NOCI(g)
Transcribed Image Text:Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl₂(g) = 2 NOCI(g)
Expert Solution
Step 1

Given data : 

At equilibrium: 

partial pressure of NO = 0.095 atm 

partial pressure of NOCl = 0.28 atm 

partial pressure of Cl2 = 0.171 atm 

The reaction : 

2 NO(g) + Cl2 (g) ==> 2NOCl (g) 

 

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