Consider the reaction: 2 NO(g) + Br₂(g) ⇌ 2 NOBr(g) A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br₂) into a sealed 1.00 L reaction vessel and then allowed the reaction to reach equilibrium. The pressure of the NOBr at equilibrium at 25.0°C is 0.444 bar. (R = 0.08314 L･bar/mol･K and MW of Br₂ is 159.808 g/mol.) Calculate the Kp.
Consider the reaction: 2 NO(g) + Br₂(g) ⇌ 2 NOBr(g) A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br₂) into a sealed 1.00 L reaction vessel and then allowed the reaction to reach equilibrium. The pressure of the NOBr at equilibrium at 25.0°C is 0.444 bar. (R = 0.08314 L･bar/mol･K and MW of Br₂ is 159.808 g/mol.) Calculate the Kp.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 62QRT
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Consider the reaction: 2 NO(g) + Br₂(g) ⇌ 2 NOBr(g) A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br₂) into a sealed 1.00 L reaction vessel and then allowed the reaction to reach equilibrium. The pressure of the NOBr at equilibrium at 25.0°C is 0.444 bar. (R = 0.08314 L･bar/mol･K and MW of Br₂ is 159.808 g/mol.) Calculate the Kp.
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