1. What is Kp?

Kp is the equilibrium constant expressed in terms of partial pressures for gas-phase reactions. It relates the partial pressures of products and reactants at equilibrium.

2. How Does the Calculator Work?

The calculator uses the Kp equilibrium expression:

Where:

• \( K_p \) — Equilibrium constant in terms of partial pressures
• \( P_A \) — Partial pressure of reactant A (atm)
• \( P_B \) — Partial pressure of product B (atm)
• \( a \) — Stoichiometric coefficient of reactant A
• \( b \) — Stoichiometric coefficient of product B

Explanation: Given Kp and one partial pressure, the calculator solves for the unknown partial pressure using algebraic rearrangement of the equilibrium expression.

3. Importance of Partial Pressures

Details: Partial pressure calculations are essential for understanding gas-phase equilibria, predicting reaction directions, and determining equilibrium yields in industrial processes.

4. Using the Calculator

Tips: Enter Kp value, stoichiometric coefficients, known partial pressure, and specify whether it's for reactant or product. All values must be positive.

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 \( K_p = K_c(RT)^{Δn} \).

Q2: What if my reaction has multiple reactants/products?
A: This calculator handles simple 1-reactant, 1-product cases. For complex reactions, extend the equilibrium expression accordingly.

Q3: What units should I use?
A: Use atm for pressures. Kp units depend on the reaction stoichiometry (atm^Δn).

Q4: Does temperature affect Kp?
A: Yes, Kp is temperature-dependent. This calculator assumes you're using a Kp value for your specific temperature.

Q5: What if my reaction goes to completion?
A: Extremely large Kp values may indicate essentially complete reactions where equilibrium calculations become less meaningful.