**Initial Concentrations and Direction to Equilibrium**This table displays the initial concentrations or pressures of reactants and products for several chemical reactions, along with their respective equilibrium constant (\(K_c\)) values. To determine the movement of each system toward equilibrium, we calculate the reaction quotient \(Q\) and compare it to the equilibrium constant \(K_c\). | Reaction | \(K_c\) value | Concentrations ||----------|---------------|----------------|| \(2\text{NH}_3 (g) \leftrightarrow \text{N}_2 (g) + 3\text{H}_2 (g)\) | 17 | \([\text{NH}_3] = 0.20\text{ M}, [\text{N}_2] = 1.00\text{ M}, [\text{H}_2] = 1.00\text{ M}\) || \(2\text{NH}_3 (g) \leftrightarrow \text{N}_2 (g) + 3\text{H}_2 (g)\) | \(6.8 \times 10^4\) | \(\text{NH}_3 = 3.0\text{ atm}, \text{N}_2 = 2.0\text{ atm}, \text{H}_2 = 1.0\text{ atm}\) || \(2\text{SO}_3 (g) \leftrightarrow 2\text{SO}_2 (g) + \text{O}_2 (g)\) | 0.230 | \([\text{SO}_3] = 0.00\text{ M}, [\text{SO}_2] = 1.00\text{ M}, [\text{O}_2] = 1.00\text{ M}\) |**Analysis:**1. **For the first reaction \(2\text{NH}_3 (g) \leftrightarrow \text{N}_2 (g) + 3\text{H}_2 (g)\) with \(K_c = 17\):** - **Given concentrations:** \([\text{NH}_3] = 0.20\text{ M}, [\text{N}_2] = 1.00\text{ M}, [

♣ The equilibrium concentration Kc is defined as the ratio of equilibrium concentration of the…

The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. Reaction Kc value Concentrations 2NH3 (9) N₂ (g) + 3H₂ (g) 17 [NH3] = 0.20 M, [N₂] = 1.00 M, [H₂] = 1.00 M 2NH3 (9) N₂ (g) + 3H₂ (g) 6.8 x 104 NH3 = 3.0 atm, N₂ = 2.0 atm, H₂ = 1.0 atm 2SO3 (g)2SO₂ (g) + O₂ (g) 0.230 [SO3] = 0.00 M, [SO₂] = 1.00 M, [O₂] = 1.00 M

The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. Reaction Kc value Concentrations 2NH3 (9) N₂ (g) + 3H₂ (g) 17 [NH3] = 0.20 M, [N₂] = 1.00 M, [H₂] = 1.00 M 2NH3 (9) N₂ (g) + 3H₂ (g) 6.8 x 104 NH3 = 3.0 atm, N₂ = 2.0 atm, H₂ = 1.0 atm 2SO3 (g)2SO₂ (g) + O₂ (g) 0.230 [SO3] = 0.00 M, [SO₂] = 1.00 M, [O₂] = 1.00 M

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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Question

**Initial Concentrations and Direction to Equilibrium**

This table displays the initial concentrations or pressures of reactants and products for several chemical reactions, along with their respective equilibrium constant (\(K_c\)) values. To determine the movement of each system toward equilibrium, we calculate the reaction quotient \(Q\) and compare it to the equilibrium constant \(K_c\).

| Reaction | \(K_c\) value | Concentrations |
|----------|---------------|----------------|
| \(2\text{NH}_3 (g) \leftrightarrow \text{N}_2 (g) + 3\text{H}_2 (g)\) | 17 | \([\text{NH}_3] = 0.20\text{ M}, [\text{N}_2] = 1.00\text{ M}, [\text{H}_2] = 1.00\text{ M}\) |
| \(2\text{NH}_3 (g) \leftrightarrow \text{N}_2 (g) + 3\text{H}_2 (g)\) | \(6.8 \times 10^4\) | \(\text{NH}_3 = 3.0\text{ atm}, \text{N}_2 = 2.0\text{ atm}, \text{H}_2 = 1.0\text{ atm}\) |
| \(2\text{SO}_3 (g) \leftrightarrow 2\text{SO}_2 (g) + \text{O}_2 (g)\) | 0.230 | \([\text{SO}_3] = 0.00\text{ M}, [\text{SO}_2] = 1.00\text{ M}, [\text{O}_2] = 1.00\text{ M}\) |

**Analysis:**

1. **For the first reaction \(2\text{NH}_3 (g) \leftrightarrow \text{N}_2 (g) + 3\text{H}_2 (g)\) with \(K_c = 17\):**
- **Given concentrations:** \([\text{NH}_3] = 0.20\text{ M}, [\text{N}_2] = 1.00\text{ M}, [

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