A student ran the following reaction in the laboratory at 677 K: H2(g) + I2(g) 2HI(g) When she introduced H2(g) and I2(g) into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.56 atm and the initial partial pressure of I2 was 3.56 atm, she found that the equilibrium partial pressure of I2 was 0.450 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp =
A student ran the following reaction in the laboratory at 677 K: H2(g) + I2(g) 2HI(g) When she introduced H2(g) and I2(g) into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.56 atm and the initial partial pressure of I2 was 3.56 atm, she found that the equilibrium partial pressure of I2 was 0.450 atm. Calculate the equilibrium constant, Kp, she 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 97QRT
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A student ran the following reaction in the laboratory at 677 K:
H2(g) + I2(g) 2HI(g)
When she introduced H2(g) and I2(g) into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.56 atm and the initial partial pressure of I2 was 3.56 atm, she found that the equilibrium partial pressure of I2 was 0.450 atm.
Calculate the equilibrium constant, Kp, she obtained for this reaction.
Kp =
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