1. What is Equilibrium Constant with respect to Pressure?

Definition: The equilibrium constant (K_p) relates the partial pressures of reactants and products at equilibrium for gas-phase reactions.

Purpose: It helps chemists understand the extent of a chemical reaction at equilibrium under specific pressure conditions.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( K_p \) — Equilibrium constant (mol/m³)
• \( P \) — Pressure (Pascal)
• \( \alpha \) — Degree of dissociation (unitless, between 0 and 1)

Explanation: The formula calculates the equilibrium constant based on the system pressure and the fraction of molecules that dissociate.

3. Importance of Equilibrium Constant Calculation

Details: Knowing K_p helps predict reaction direction, equilibrium positions, and optimize industrial chemical processes.

4. Using the Calculator

Tips: Enter the system pressure in Pascals and degree of dissociation (between 0 and 1). The degree of dissociation must be less than 1.

5. Frequently Asked Questions (FAQ)

Q1: What does the degree of dissociation represent?
A: It's the fraction of reactant molecules that dissociate into products at equilibrium.

Q2: Why must α be less than 1?
A: A value of 1 would mean complete dissociation, making the denominator zero (undefined).

Q3: How does pressure affect K_p?
A: K_p is pressure-dependent - increasing pressure typically shifts equilibrium toward the side with fewer gas molecules.

Q4: What are typical K_p values?
A: Values vary widely - very small for reactions that barely proceed, very large for reactions that go nearly to completion.

Q5: Can I use this for liquid-phase reactions?
A: No, this calculator is specifically for gas-phase reactions where partial pressures are relevant.