### Equilibrium Concentration Calculation#### Chemical Reaction:\[ \text{SO}_2(g) + \text{Cl}_2(g) \rightleftharpoons \text{SO}_2\text{Cl}_2(g) \]- **Enthalpy Change (\(\Delta H^\circ\))**: \(-264 \, \text{kJ}\)- **Equilibrium Constant (K)**: \(34.5\)#### Given Data:At \(300 \, \text{K}\), the equilibrium concentrations are:- \([\text{SO}_2] = 0.65 \, \text{M}\)- \([\text{Cl}_2] = 0.85 \, \text{M}\)#### Problem Statement:What is the equilibrium concentration of \(\text{SO}_2\text{Cl}_2\) at this temperature?\[ [\text{SO}_2\text{Cl}_2] = [?] \, \text{M} \]Below the problem statement, there is a text box where the concentration of \(\text{SO}_2\text{Cl}_2\) can be entered with an "Enter" button beside it.#### Explanation:To find the equilibrium concentration of \(\text{SO}_2\text{Cl}_2\), you can use the expression for the equilibrium constant \(K\):\[ K = \frac{[\text{SO}_2\text{Cl}_2]}{[\text{SO}_2][\text{Cl}_2]} \]Rearranging this equation to solve for \( [\text{SO}_2\text{Cl}_2] \) gives:\[ [\text{SO}_2\text{Cl}_2] = K \times [\text{SO}_2] \times [\text{Cl}_2] \]Substitute the given values into the equation to calculate the equilibrium concentration of \(\text{SO}_2\text{Cl}_2\).

Here we are required to find the equilibrium concentration of SO2Cl2

SO₂(g) + Cl₂(g) = SO₂Cl₂(g) ΔΗ° = −264 kJ K = 34.5 At 300 K, a set of equilibrium concentrations are 0.65 M for SO2 and 0.85 M for Cl2. What is the equilibrium concentration of SO2Cl2 at this temperature? [SO₂Cl₂] = [?] M [SO,CI₂] M Enter

SO₂(g) + Cl₂(g) = SO₂Cl₂(g) ΔΗ° = −264 kJ K = 34.5 At 300 K, a set of equilibrium concentrations are 0.65 M for SO2 and 0.85 M for Cl2. What is the equilibrium concentration of SO2Cl2 at this temperature? [SO₂Cl₂] = [?] M [SO,CI₂] M Enter

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

### Equilibrium Concentration Calculation

#### Chemical Reaction:
\[ \text{SO}_2(g) + \text{Cl}_2(g) \rightleftharpoons \text{SO}_2\text{Cl}_2(g) \]

- **Enthalpy Change (\(\Delta H^\circ\))**: \(-264 \, \text{kJ}\)
- **Equilibrium Constant (K)**: \(34.5\)

#### Given Data:
At \(300 \, \text{K}\), the equilibrium concentrations are:
- \([\text{SO}_2] = 0.65 \, \text{M}\)
- \([\text{Cl}_2] = 0.85 \, \text{M}\)

#### Problem Statement:
What is the equilibrium concentration of \(\text{SO}_2\text{Cl}_2\) at this temperature?

\[ [\text{SO}_2\text{Cl}_2] = [?] \, \text{M} \]

Below the problem statement, there is a text box where the concentration of \(\text{SO}_2\text{Cl}_2\) can be entered with an "Enter" button beside it.

#### Explanation:
To find the equilibrium concentration of \(\text{SO}_2\text{Cl}_2\), you can use the expression for the equilibrium constant \(K\):

\[ K = \frac{[\text{SO}_2\text{Cl}_2]}{[\text{SO}_2][\text{Cl}_2]} \]

Rearranging this equation to solve for \( [\text{SO}_2\text{Cl}_2] \) gives:

\[ [\text{SO}_2\text{Cl}_2] = K \times [\text{SO}_2] \times [\text{Cl}_2] \]

Substitute the given values into the equation to calculate the equilibrium concentration of \(\text{SO}_2\text{Cl}_2\).

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