Math Problem Statement

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

Solution

The image shows the following chemical equation:

H2CO3(aq)2H+(aq)+CO32(aq)\text{H}_2\text{CO}_3 (aq) \rightleftharpoons 2\text{H}^+ (aq) + \text{CO}_3^{2-} (aq)

To write the equilibrium constant expression KcK_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 KcK_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 KcK_c and KpK_p, the equilibrium constant for partial pressures?
  4. How does temperature affect the value of KcK_c?
  5. What are the units of KcK_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 KcK_c expression.