1. What is Equilibrium Constant with respect to Pressure?

Definition: The equilibrium constant (Kₚ) is the ratio of the partial pressures of products to reactants at equilibrium, each raised to the power of their stoichiometric coefficients.

Purpose: It helps chemists understand and predict the behavior of gaseous systems at equilibrium under different pressure conditions.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( K_p \) — Equilibrium constant for partial pressure (mol/m³)
• \( P_{abs} \) — Absolute pressure (Pa)
• \( \alpha \) — Degree of dissociation (0 to 1)

Explanation: The equilibrium constant is calculated by multiplying the absolute pressure by the square of the degree of dissociation.

3. Importance of Equilibrium Constant Calculation

Details: Understanding Kₚ is crucial for predicting reaction direction, extent of reaction, and how systems respond to pressure changes (Le Chatelier's Principle).

4. Using the Calculator

Tips: Enter the absolute pressure in Pascals and degree of dissociation (between 0 and 1). All values must be > 0.

5. Frequently Asked Questions (FAQ)

Q1: What is degree of dissociation?
A: It's the fraction of reactant molecules that dissociate into products at equilibrium (0 = no dissociation, 1 = complete dissociation).

Q2: Why is the degree of dissociation squared?
A: The square comes from the stoichiometric coefficients in the equilibrium expression for a simple dissociation reaction.

Q3: How does pressure affect Kₚ?
A: Kₚ itself is constant at a given temperature, but changing pressure affects the position of equilibrium and degree of dissociation.

Q4: What are typical units for Kₚ?
A: Units depend on the reaction, but commonly mol/m³ or atmⁿ where n is the change in moles of gas.

Q5: Does this work for all reactions?
A: This specific formula applies to simple dissociation reactions. More complex reactions require different equilibrium expressions.