Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to reach equilibrium? SO₂Cl2 (8) SO2 (g) + Cl₂ (8) where [SO₂Cl₂] = 0.12 M, [Cl₂] = 0.16 M and [SO₂] = 0.050 M K for the reaction = 0.078
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Bronsted Lowry Base In Inorganic Chemistry
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![### Chemical Equilibrium Problem
**Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to reach equilibrium?**
\[ \text{SO}_2\text{Cl}_2 \, (g) \leftrightarrow \text{SO}_2 \, (g) + \text{Cl}_2 \, (g) \]
**where:**
\[ [\text{SO}_2\text{Cl}_2] = 0.12 \, M, \quad [\text{Cl}_2] = 0.16 \, M, \quad [\text{SO}_2] = 0.050 \, M \]
**Equilibrium constant (\( K_c \)) for the reaction = 0.078**
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To determine if the system is at equilibrium, we need to compare the reaction quotient (\( Q \)) to the equilibrium constant (\( K_c \)).
**Step-by-Step Solution:**
1. **Write the Expression for the Reaction Quotient, \( Q \):**
\[
Q = \frac{[\text{SO}_2][\text{Cl}_2]}{[\text{SO}_2\text{Cl}_2]}
\]
2. **Substitute the Given Concentrations into the \( Q \) Expression:**
\[
Q = \frac{(0.050)(0.16)}{0.12}
\]
3. **Calculate \( Q \):**
\[
Q = \frac{0.008}{0.12} = 0.067
\]
4. **Compare \( Q \) and \( K_c \):**
- If \( Q < K_c \): The system is not at equilibrium, and the reaction will need to shift to the right (towards the products) to reach equilibrium.
- If \( Q > K_c \): The system is not at equilibrium, and the reaction will need to shift to the left (towards the reactants) to reach equilibrium.
- If \( Q = K_c \): The system is at equilibrium.
Given:
\[ Q = 0.067 \]
\[ K_c = 0.078 \]
Since \( Q < K_c \), the system is not at equilibrium and will need to shift to the right (towards the products) to reach](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff90913a8-510d-485a-8226-8a0b61f2c858%2F23b21f93-2a2e-45ed-b42f-7a93945788eb%2F2a2z0f9_processed.png&w=3840&q=75)
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