A student ran the following reaction in the laboratory at 1090 K: ? 2SO₂(g) + O₂(g) 22SO3(9) When he introduced SO₂(g) and O₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of SO₂ was 4.68 atm and the initial partial pressure of O₂ was 2.05 atm, he found that the equilibrium partial pressure of SO3 was 2.34 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group attempts remaining
A student ran the following reaction in the laboratory at 1090 K: ? 2SO₂(g) + O₂(g) 22SO3(9) When he introduced SO₂(g) and O₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of SO₂ was 4.68 atm and the initial partial pressure of O₂ was 2.05 atm, he found that the equilibrium partial pressure of SO3 was 2.34 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group attempts remaining
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 90E: In a 3.0-L vessel, the following equilibrium partial pressures are measured: N2, 190 torr; H2, 317...
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