1. What is Kp to Kc Conversion?

The Kp to Kc conversion relates the equilibrium constant in terms of partial pressures (Kp) to the equilibrium constant in terms of concentrations (Kc). This conversion is essential in chemical equilibrium calculations, especially for gas-phase reactions.

2. How Does the Calculator Work?

The calculator uses the conversion formula:

Where:

• \( K_p \) — Equilibrium constant in terms of partial pressures
• \( K_c \) — Equilibrium constant in terms of concentrations
• \( R \) — Gas constant (0.0821 L·atm·K⁻¹·mol⁻¹)
• \( T \) — Temperature in Kelvin
• \( \Delta n \) — Change in moles of gas (products - reactants)

Explanation: The equation accounts for the relationship between pressure and concentration through the ideal gas law.

3. Importance of Kc Calculation

Details: Kc is particularly useful when working with solution concentrations or when comparing equilibrium constants for reactions under different conditions.

4. Using the Calculator

Tips: Enter Kp (must be positive), Δn (can be positive or negative), and temperature in Kelvin (must be positive). 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 of gases, while Kc uses molar concentrations. They're related through the ideal gas law.

Q2: When should I use Kc instead of Kp?
A: Use Kc when working with concentrations in solution or when comparing reactions in the same solvent. Kp is more appropriate for gas-phase reactions.

Q3: What if Δn = 0?
A: When Δn = 0, Kp = Kc because (RT)^0 = 1. This occurs when the number of moles of gas is the same on both sides.

Q4: What units should I use for temperature?
A: Temperature must be in Kelvin for this calculation. Convert from Celsius by adding 273.15.

Q5: Can this be used for all gas-phase reactions?
A: This assumes ideal gas behavior. For real gases at high pressures or low temperatures, deviations may occur.