https://file.aiquickdraw.com/mathbot/file/1727749101838m6eh946i.jpg

The image shows the following chemical equation:

\[
\text{H}_2\text{CO}_3 (aq) \rightleftharpoons 2\text{H}^+ (aq) + \text{CO}_3^{2-} (aq)
\]

To write the equilibrium constant expression \( K_c \) for this reaction, we follow this general rule:

\[
K_c = \frac{\text{[Products]}}{\text{[Reactants]}}
\]

Each concentration term is raised to the power of its stoichiometric coefficient.

For this reaction, the equilibrium constant expression is:

\[
K_c = \frac{[\text{H}^+]^2 [\text{CO}_3^{2-}]}{[\text{H}_2\text{CO}_3]}
\]

### Would you like more details or have any questions?

Here are five related questions for practice:
1. What does a high equilibrium constant \( K_c \) indicate about the position of equilibrium?
2. How do you find the equilibrium concentrations of products and reactants experimentally?
3. What is the relationship between \( K_c \) and \( K_p \), the equilibrium constant for partial pressures?
4. How does temperature affect the value of \( K_c \)?
5. What are the units of \( K_c \) for this reaction?

### Tip: 
Always pay attention to the physical states (solid, liquid, gas, aqueous) when writing equilibrium expressions, as solids and pure liquids are not included in the \( K_c \) expression.

Write the equilibrium constant expression for the reaction H₂CO₃(aq) → 2H⁺(aq) + CO₃²⁻(aq).

Learn how to write the equilibrium constant expression for the reaction H₂CO₃(aq) → 2H⁺(aq) + CO₃²⁻(aq). This example covers key concepts in chemical equilibrium, suitable for high school students.

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