Find K and average K **Transcription of Beaker C Equilibrium Experiment Data****Section 3. From Beaker C**| | Fe³⁺ | + | SCN⁻ | ⇌ | FeSCN²⁺ ||----------------------|-----------------------|------------------|---------------------|-----------------|-------------------|| **Initial** | 0.6 x 10⁻³ | | 1 x 10⁻³ | | 0 || **Change** | -9.732 x 10⁻⁵ | + | -9.732 x 10⁻⁵ | | + || **Equilibrium** | 0.898 x 10⁻³ | | 9.732 x 10⁻⁵ | | 0 |**K =** **Average K = ______****Explanation:**This table outlines the changes in concentration of the reactants and products during a chemical equilibrium experiment involving iron(III) ions (Fe³⁺), thiocyanate ions (SCN⁻), and the resulting complex ion (FeSCN²⁺). The concentrations are given in molarity (M).- **Initial Row:** Shows the starting concentrations of Fe³⁺ and SCN⁻, with FeSCN²⁺ initially being 0 M.- **Change Row:** Indicates the change in concentration needed to reach equilibrium. The reactants decrease by 9.732 x 10⁻⁵ M, suggesting formation of FeSCN²⁺.- **Equilibrium Row:** Displays the concentrations when the system reaches equilibrium.The blank areas under “K” and “Average K” are likely for calculating the equilibrium constant (K) based on the given data.

Answered: Image /qna-images/answer/f9241410-7dd2-4ddf-a242-95849a341da0.jpg

Answered: 3. From Beaker C K= Initial Change…

3. From Beaker C K= Initial Change Equilibrium Average K= Fe³+ 0.6x10 3 -9.732x10-5 0.899x103 + SCN 1x10³ +9.732x105 9.73240² FeSCN2+ 0 0 0

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

Find K and average K

**Transcription of Beaker C Equilibrium Experiment Data**

**Section 3. From Beaker C**

| | Fe³⁺ | + | SCN⁻ | ⇌ | FeSCN²⁺ |
|----------------------|-----------------------|------------------|---------------------|-----------------|-------------------|
| **Initial** | 0.6 x 10⁻³ | | 1 x 10⁻³ | | 0 |
| **Change** | -9.732 x 10⁻⁵ | + | -9.732 x 10⁻⁵ | | + |
| **Equilibrium** | 0.898 x 10⁻³ | | 9.732 x 10⁻⁵ | | 0 |

**K =**
**Average K = ______**

**Explanation:**

This table outlines the changes in concentration of the reactants and products during a chemical equilibrium experiment involving iron(III) ions (Fe³⁺), thiocyanate ions (SCN⁻), and the resulting complex ion (FeSCN²⁺). The concentrations are given in molarity (M).

- **Initial Row:** Shows the starting concentrations of Fe³⁺ and SCN⁻, with FeSCN²⁺ initially being 0 M.
- **Change Row:** Indicates the change in concentration needed to reach equilibrium. The reactants decrease by 9.732 x 10⁻⁵ M, suggesting formation of FeSCN²⁺.
- **Equilibrium Row:** Displays the concentrations when the system reaches equilibrium.

The blank areas under “K” and “Average K” are likely for calculating the equilibrium constant (K) based on the given data.

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