1. What is Kp and Kc?

Kp and Kc are equilibrium constants for gas-phase reactions. Kc is based on concentrations (mol/L), while Kp is based on partial pressures (atm). The relationship between them is given by the formula Kp = Kc (RT)^Δn.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( K_c \) — Equilibrium constant based on concentrations (unitless)
• \( R \) — Gas constant (0.0821 L atm/mol K)
• \( T \) — Temperature in Kelvin (K)
• \( \Delta n \) — Change in number of moles of gas (unitless)

Explanation: The equation converts between concentration-based and pressure-based equilibrium constants using the ideal gas law relationship.

3. Importance of Kp Calculation

Details: Calculating Kp from Kc is essential for understanding gas-phase equilibria and for comparing equilibrium constants measured under different conditions.

4. Using the Calculator

Tips: Enter Kc (unitless), R (typically 0.0821 L atm/mol K), temperature in Kelvin, and Δn (change in moles of gas). All values must be valid.

5. Frequently Asked Questions (FAQ)

Q1: What is Δn in the formula?
A: Δn is the difference between the sum of stoichiometric coefficients of gaseous products and reactants (Δn = Σn_products - Σn_reactants).

Q2: When should I use Kp instead of Kc?
A: Use Kp when dealing with gas-phase reactions where partial pressures are more convenient or measurable than concentrations.

Q3: What are typical values for Kp and Kc?
A: Both can range from very small to very large values, indicating the extent of reaction at equilibrium.

Q4: Are there limitations to this conversion?
A: This conversion assumes ideal gas behavior and may not be accurate at high pressures or for real gases.

Q5: Can this be used for reactions involving both gases and other phases?
A: The conversion only applies to gaseous components. Solids and liquids are not included in Δn calculations.