**Calculating an Equilibrium Constant from a Heterogeneous Reaction**Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, as shown in the equation:\[ 3 \text{NO}_2(g) + \text{H}_2\text{O}(l) \rightarrow 2 \text{HNO}_3(aq) + \text{NO}(g) \]At a certain temperature, a chemist finds that a 5.6 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition:| Compound | Amount (g) ||----------|------------|| NO₂ | 193.8 || H₂O | 212.3 || HNO₃ | 184.5 || NO | 21.1 |Calculate the value of the equilibrium constant \( K_c \) for this reaction. Round your answer to 2 significant digits.\[ K_c = \]There’s a placeholder box to enter the calculated value of \( K_c \).- **Explanation:** A section is available for detailed explanations.- **Check:** There’s a button to check the answer.---This educational problem guides the student through calculating an equilibrium constant from provided data, emphasizing understanding equilibrium in chemical reactions.

Answered: Nitrogen dioxide and water react to…

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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**Calculating an Equilibrium Constant from a Heterogeneous Reaction**

Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, as shown in the equation:

\[ 3 \text{NO}_2(g) + \text{H}_2\text{O}(l) \rightarrow 2 \text{HNO}_3(aq) + \text{NO}(g) \]

At a certain temperature, a chemist finds that a 5.6 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition:

| Compound | Amount (g) |
|----------|------------|
| NO₂ | 193.8 |
| H₂O | 212.3 |
| HNO₃ | 184.5 |
| NO | 21.1 |

Calculate the value of the equilibrium constant \( K_c \) for this reaction. Round your answer to 2 significant digits.

\[ K_c = \]

There’s a placeholder box to enter the calculated value of \( K_c \).

- **Explanation:** A section is available for detailed explanations.
- **Check:** There’s a button to check the answer.

---

This educational problem guides the student through calculating an equilibrium constant from provided data, emphasizing understanding equilibrium in chemical reactions.

Expert Solution

Step 1

The equilibrium constant (Kc) of a reaction is the ratio of product of molar concentrations of products to that of reactants where their respective coefficients in the balanced chemical reaction become exponents of their concentrations.

Given:

Mass of NO₂is 19.3 g.

Mass of H₂O is 212.3 g.

Mass of HNO₃ is 18.4 g.

Mass of NO is 21.1 g.

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