Degree of Dissociation when Pressure Increases during Reaction Calculator

Degree of Dissociation Formula:

\[ \alpha = \sqrt{\frac{K_p}{P}} \]

Degree of Dissociation (α):

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1. What is Degree of Dissociation when Pressure Increases?

Definition: The degree of dissociation (α) measures the fraction of molecules that dissociate into ions or smaller molecules at equilibrium.

Purpose: This calculator determines how pressure changes affect the dissociation of molecules in a chemical reaction at equilibrium.

2. How Does the Calculator Work?

The calculator uses the formula:

\[ \alpha = \sqrt{\frac{K_p}{P}} \]

Where:

\( \alpha \) — Degree of dissociation (unitless, between 0 and 1)
\( K_p \) — Equilibrium constant for partial pressure (mol/m³)
\( P \) — Total pressure (Pa)

Explanation: The degree of dissociation decreases with increasing pressure, following Le Chatelier's principle.

3. Importance of Degree of Dissociation

Details: Understanding dissociation helps predict reaction behavior, equilibrium shifts, and optimize industrial chemical processes.

4. Using the Calculator

Tips: Enter the equilibrium constant (K_p) and the system pressure. Both values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: Why does dissociation decrease with pressure?
A: According to Le Chatelier's principle, systems shift to reduce pressure increases, favoring the side with fewer gas molecules.

Q2: What's the range for degree of dissociation?
A: α ranges from 0 (no dissociation) to 1 (complete dissociation).

Q3: Does this formula work for all reactions?
A: No, it's specific for reactions where the number of gas molecules increases during dissociation.

Q4: How do I find K_p values?
A: K_p can be calculated from standard Gibbs free energy or measured experimentally.

Q5: What units should I use?
A: Use consistent units (mol/m³ for K_p and Pa for pressure) for accurate results.