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The following reaction is important in the manufacture of sulfuric acid: SO2 (9) + 02 (9) = SO3 (9) At a certain temperature, 1.39 x 10¬² mol of SO2 and 3.30 x 10-2 mol of O2 are sealed in a 1.00-L reaction vessel. When equilibrium is reached, the concentration of SO3 is determined to be 1.22 × 10-² M. Calculate K. for this reaction. Ke =

The following reaction is important in the manufacture of sulfuric acid: SO2 (9) + 02 (9) = SO3 (9) At a certain temperature, 1.39 x 10¬² mol of SO2 and 3.30 x 10-2 mol of O2 are sealed in a 1.00-L reaction vessel. When equilibrium is reached, the concentration of SO3 is determined to be 1.22 × 10-² M. Calculate K. for this reaction. Ke =

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.40QE
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The following reaction is important in the manufacture of sulfuric acid: SO: (9) + 02 (9) = SO3 (g) At a certain temperature, 1.39 × 10-2 mol of SO2 and 3.30 x 10-2 mol of O2 are sealed in a 1.00-L reaction vessel. When equilibrium is reached, the concentration of SO3 is determined to be 1.22 × 10-2 M. Calculate K. for this reaction. K. =
Transcribed Image Text:The following reaction is important in the manufacture of sulfuric acid: SO: (9) + 02 (9) = SO3 (g) At a certain temperature, 1.39 × 10-2 mol of SO2 and 3.30 x 10-2 mol of O2 are sealed in a 1.00-L reaction vessel. When equilibrium is reached, the concentration of SO3 is determined to be 1.22 × 10-2 M. Calculate K. for this reaction. K. =
A student ran the following reaction in the laboratory at 744 K: H2(g) + I2(g)=2HI(g) When she introduced 0.193 moles of H,(g) and 0.225 moles of I,(g) into a 1.00 liter container, she found the equilibrium concentration of I,(g) to be 6.41x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =
Transcribed Image Text:A student ran the following reaction in the laboratory at 744 K: H2(g) + I2(g)=2HI(g) When she introduced 0.193 moles of H,(g) and 0.225 moles of I,(g) into a 1.00 liter container, she found the equilibrium concentration of I,(g) to be 6.41x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =
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