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: 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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