4 **Equilibrium in Chemical Reactions**In this lesson, we will explore how to determine the equilibrium constant for a chemical reaction. As an example, consider the following reaction where nitrogen dioxide and water react to form nitric acid and nitrogen monoxide:\[ 3 \text{NO}_2(g) + \text{H}_2\text{O}(l) \rightarrow 2 \text{HNO}_3(aq) + \text{NO}(g) \]At a certain temperature, a chemist observes a 4.0 L reaction vessel containing a mixture of these substances at equilibrium with the following composition:| Compound | Amount ||----------|--------|| NO$_2$ | 18.3 g || H$_2$O | 73.9 g || HNO$_3$| 5.0 g || NO | 14.7 g |To calculate the equilibrium constant ($K_c$) for this reaction, follow these steps:1. **Convert Mass to Moles**: Calculate the number of moles for each compound using their molar mass. - Molar mass of NO$_2$ = 14 (N) + 2×16 (O) = 46 g/mol - Molar mass of H$_2$O = 2×1 (H) + 16 (O) = 18 g/mol - Molar mass of HNO$_3$ = 1 (H) + 14 (N) + 3×16 (O) = 63 g/mol - Molar mass of NO = 14 (N) + 16 (O) = 30 g/mol2. **Calculate Concentrations (M)**: Convert moles to molarity by dividing by the volume of the reaction vessel (4.0 L).3. **Determine $K_c$ Using the Equilibrium Expression**: The equilibrium constant expression for the reaction is: \[ K_c = \frac{[\text{HNO}_3]^2 [\text{NO}]}{[\text{NO}_2]^3 [\text{H}_2\text{O}]} \]4. **Insert Concentrations and Solve**: Use the concentrations computed in the previous step to find $K_c$.

Answered: Image /qna-images/answer/af58824f-c412-4a63-98cd-578a0188e590.jpg

Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(g) + H₂O(1)→ 2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 18.3 g H₂O 73.9 g HNO3 5.0 g NO 14.7 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K x10

Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(g) + H₂O(1)→ 2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 18.3 g H₂O 73.9 g HNO3 5.0 g NO 14.7 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K x10

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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