1. What is the Kp Calculation?

The Kp calculation converts the equilibrium constant Kc (based on concentrations) to Kp (based on partial pressures) using the ideal gas law. This is essential for gas-phase reactions where pressures are more easily measured than concentrations.

2. How Does the Calculator Work?

The calculator uses the Kp equation:

Where:

• \( K_p \) — Equilibrium constant in terms of partial pressures (unitless)
• \( K_c \) — Equilibrium constant in terms of concentrations (unitless)
• \( R \) — Gas constant (0.0821 L·atm/(mol·K))
• \( T \) — Temperature in Kelvin (K)
• \( \Delta n \) — Change in moles of gas (products - reactants)

Explanation: The equation accounts for the relationship between concentration and pressure in gas-phase reactions at equilibrium.

3. Importance of Kp Calculation

Details: Kp is crucial for understanding gas-phase equilibria, predicting reaction directions, and calculating equilibrium pressures in industrial chemical processes.

4. Using the Calculator

Tips: Enter Kc (must be positive), temperature in Kelvin (must be positive), and Δn (can be positive, negative, or zero). All values must be valid 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 through the ideal gas law and are equal when Δn = 0.

Q2: How do I determine Δn?
A: Δn = (total moles of gaseous products) - (total moles of gaseous reactants) from the balanced equation.

Q3: What units should I use for temperature?
A: Temperature must be in Kelvin (K). Convert from Celsius by adding 273.15.

Q4: When is Kp equal to Kc?
A: When Δn = 0 (same number of moles of gas on both sides of the equation).

Q5: Can this be used for non-gas reactions?
A: No, Kp is only meaningful for reactions involving gases. For aqueous reactions, use Kc.