https://file.aiquickdraw.com/mathbot/file/1727749213153ypxi1g8n.jpg

To write the equilibrium constant expression for the given reaction:

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

The equilibrium constant expression (\(K_c\)) is based on the concentrations of the products and reactants at equilibrium. The general form of the equilibrium constant expression for a reaction:

\[
aA + bB \rightleftharpoons cC + dD
\]

is given by:

\[
K_c = \frac{[\text{C}]^c [\text{D}]^d}{[\text{A}]^a [\text{B}]^b}
\]

For your reaction:

- Products: \(2 \text{H}^+ (aq)\) and \(\text{CO}_3^{2-} (aq)\)
- Reactant: \(\text{H}_2\text{CO}_3 (aq)\)

Thus, the equilibrium constant expression will be:

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

Do you have any other questions about this? Would you like further details?

Here are some related questions for further study:
1. How do changes in concentration affect the equilibrium position of this reaction?
2. What is the role of \(K_c\) in determining whether the forward or reverse reaction is favored?
3. How would the equilibrium constant expression change for a different reaction?
4. What happens to the equilibrium constant when the temperature changes?
5. What are the units of the equilibrium constant for this reaction?

**Tip:** Remember that \(K_c\) expressions only include species that are in the aqueous or gaseous state, not solids or liquids!

Write the equilibrium constant expression for this 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 problem covers core chemistry concepts, including stoichiometry and equilibrium expressions, suitable for high school chemistry students.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation