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A student ran the following reaction in the laboratory at 696 K: 2HI(g) H2(g) + I2(g) When he introduced HI(g) at a pressure of 3.40 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 2.68 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Кр

A student ran the following reaction in the laboratory at 696 K: 2HI(g) H2(g) + I2(g) When he introduced HI(g) at a pressure of 3.40 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 2.68 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Кр

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter19: The Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 60QRT
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A student ran the following reaction in the laboratory at 696 K: 2HI(g) H2(g) + I2(g) When he introduced HI(g) at a pressure of 3.40 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 2.68 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp =
Transcribed Image Text:A student ran the following reaction in the laboratory at 696 K: 2HI(g) H2(g) + I2(g) When he introduced HI(g) at a pressure of 3.40 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 2.68 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp =
A student ran the following reaction in the laboratory at 594 K: Co(g) + Cl2(g) =cOCl2(g) When she introduced CO(g) and Cl2(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.26 atm and the initial partial pressure of Cl2 was 1.35 atm, she found that the equilibrium partial pressure of Cl2 was 0.381 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp %D
Transcribed Image Text:A student ran the following reaction in the laboratory at 594 K: Co(g) + Cl2(g) =cOCl2(g) When she introduced CO(g) and Cl2(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.26 atm and the initial partial pressure of Cl2 was 1.35 atm, she found that the equilibrium partial pressure of Cl2 was 0.381 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp %D
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