1. What is Kp?

Kp is the equilibrium constant calculated from the partial pressures of gases in a chemical reaction at equilibrium. It relates the partial pressures of products to reactants, raised to their stoichiometric coefficients.

2. How Does the Calculator Work?

The calculator uses the Kp formula:

Where:

• Product Partial Pressures — Sum of partial pressures of all products
• Reactant Partial Pressures — Sum of partial pressures of all reactants

Explanation: For a general reaction aA + bB ⇌ cC + dD, the Kp expression would be (PC^c × PD^d)/(PA^a × PB^b).

3. Importance of Kp Calculation

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

4. Using the Calculator

Tips: Enter the total partial pressures of products and reactants in atm (atmospheres). Reactant pressure must be greater than zero.

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, where Δn is the change in moles of gas.

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: Does Kp change with temperature?
A: Yes, Kp is temperature-dependent. It changes according to the van't Hoff equation when temperature changes.

Q4: What are the units of Kp?
A: Kp is technically dimensionless when using standard state pressure (1 atm), though the calculation involves pressure units that cancel out.

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