1. What is the Pressure Equilibrium Constant?

The pressure equilibrium constant (Kp) relates the partial pressures of products and reactants at equilibrium in a gaseous chemical reaction. It is a dimensionless quantity that indicates the extent of a reaction at equilibrium.

2. How Does the Calculator Work?

The calculator uses the Kp equation:

Where:

• Partial pressures are in atmospheres (atm)
• Each partial pressure is raised to the power of its stoichiometric coefficient
• Kp is dimensionless

Explanation: The equation shows the ratio of product pressures to reactant pressures at equilibrium.

3. Importance of Kp Calculation

Details: Kp helps predict the direction of a reaction, determine equilibrium concentrations, and understand how changes in conditions affect the equilibrium position.

4. Using the Calculator

Tips: Enter the product of partial pressures of products and reactants in atm. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: What's the difference between Kp and Kc?
A: Kp uses partial pressures while Kc uses concentrations. They're related by the equation Kp = Kc(RT)^Δn.

Q2: What does a large Kp value indicate?
A: A large Kp (>1) means products are favored at equilibrium, while a small Kp (<1) means reactants are favored.

Q3: How does temperature affect Kp?
A: Kp changes with temperature - it increases for endothermic reactions and decreases for exothermic reactions as temperature rises.

Q4: What are the units of Kp?
A: Kp is technically dimensionless, though the partial pressures used in its calculation are typically in atm.

Q5: Can Kp be used for liquids or solids?
A: No, Kp is only for gas-phase reactions. Pure liquids and solids are not included in Kp expressions.