1. What is Kp?

Kp is the equilibrium constant expressed in terms of partial pressures. It is used for gas-phase reactions and represents the ratio of product partial pressures to reactant partial pressures, each raised to the power of their stoichiometric coefficients.

2. How Does the Calculator Work?

The calculator uses the Kp formula:

Where:

• Product Partial Pressures — Sum of partial pressures of products (atm)
• Reactant Partial Pressures — Sum of partial pressures of reactants (atm)

Explanation: Kp provides information about the position of equilibrium for gas-phase reactions. A Kp > 1 favors products, while Kp < 1 favors reactants.

3. Importance of Kp Calculation

Details: Calculating Kp is essential for understanding chemical equilibrium in gas-phase reactions, predicting reaction direction, and determining optimal conditions for industrial processes.

4. Using the Calculator

Tips: Enter partial pressures in atm units. Ensure reactant partial pressure is greater than zero. All values must be valid non-negative 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 are related through the ideal gas law: Kp = Kc(RT)^Δn

Q2: When should I use Kp instead of Kc?
A: Use Kp for gas-phase reactions where partial pressures are more convenient to measure than concentrations.

Q3: What are typical Kp values?
A: Kp values can range from very small (10^-10) to very large (10¹⁰), indicating the extent to which a reaction proceeds.

Q4: How does temperature affect Kp?
A: Kp is temperature-dependent. For exothermic reactions, Kp decreases with increasing temperature, while for endothermic reactions, Kp increases.

Q5: Can Kp be used for reactions with solids or liquids?
A: No, Kp is specifically for gas-phase reactions. For reactions involving solids or liquids, use Kc or other appropriate equilibrium constants.