Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Equilibrium Concentrations in Chemical Reactions**
A mixture containing 0.856 moles of NO, 0.656 moles of H₂, and 1.16 moles of H₂O is placed in a 1.0-liter vessel at 300 K. The system reaches equilibrium according to the following reaction:
\[ 2\text{NO}(g) + 2\text{H}_2(g) \rightleftharpoons \text{N}_2(g) + 2\text{H}_2\text{O}(g) \]
At equilibrium, the concentration of NO is measured to be 0.248 M.
**Part A: Equilibrium Concentration of H₂**
Calculate the equilibrium concentration of H₂. Express the molarity to three decimal places.
\[ \text{Equilibrium Concentration of H}_2 = \boxed{\,\,\,}\, \, M \]
**Part B: Equilibrium Concentration of N₂**
Calculate the equilibrium concentration of N₂. Express the molarity to three decimal places.
\[ \text{Equilibrium Concentration of N}_2 = \boxed{\,\,\,}\, \, M \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1205cd08-0e41-4ad8-bd1c-6b97372ee2c1%2Fc6969f6d-cb70-4c8b-af66-2809a1a17305%2Fxoc1k2m_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Equilibrium Concentrations in Chemical Reactions**
A mixture containing 0.856 moles of NO, 0.656 moles of H₂, and 1.16 moles of H₂O is placed in a 1.0-liter vessel at 300 K. The system reaches equilibrium according to the following reaction:
\[ 2\text{NO}(g) + 2\text{H}_2(g) \rightleftharpoons \text{N}_2(g) + 2\text{H}_2\text{O}(g) \]
At equilibrium, the concentration of NO is measured to be 0.248 M.
**Part A: Equilibrium Concentration of H₂**
Calculate the equilibrium concentration of H₂. Express the molarity to three decimal places.
\[ \text{Equilibrium Concentration of H}_2 = \boxed{\,\,\,}\, \, M \]
**Part B: Equilibrium Concentration of N₂**
Calculate the equilibrium concentration of N₂. Express the molarity to three decimal places.
\[ \text{Equilibrium Concentration of N}_2 = \boxed{\,\,\,}\, \, M \]
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