A student ran the following reaction in the laboratory at 698 K:2HI(g) H2(g) + I2(g)When he introduced HI(g) at a pressure of 4.91 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.520 atm.Calculate the equilibrium constant, Kp, he obtained for this reaction.Kp =
A student ran the following reaction in the laboratory at 698 K:2HI(g) H2(g) + I2(g)When he introduced HI(g) at a pressure of 4.91 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.520 atm.Calculate the equilibrium constant, Kp, he obtained for this reaction.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 41QRT: Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures.
2 NOCl(g) ⇌ 2 NO(g) +...
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Question
A student ran the following reaction in the laboratory at 698 K:
2HI(g) H2(g) + I2(g)
When he introduced HI(g) at a pressure of 4.91 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.520 atm.
Calculate the equilibrium constant, Kp, he obtained for this reaction.
Kp =
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