1. What is Equilibrium Partial Pressure?

The equilibrium partial pressure is the pressure exerted by a gas in a mixture when the reaction has reached equilibrium. The equilibrium constant K_p relates the partial pressures of products and reactants at equilibrium.

2. How Does the Calculator Work?

The calculator uses the equilibrium expression:

Where:

• \( K_p \) — Equilibrium constant in terms of partial pressures
• \( P_{\text{products}} \) — Partial pressures of products at equilibrium
• \( P_{\text{reactants}} \) — Partial pressures of reactants at equilibrium
• coefficients — Stoichiometric coefficients from the balanced equation

Explanation: The equation shows the ratio of product pressures to reactant pressures, each raised to their stoichiometric coefficients.

3. Importance of K_p Calculation

Details: Calculating equilibrium partial pressures is essential for understanding chemical equilibria in gas-phase reactions, predicting reaction outcomes, and designing industrial chemical processes.

4. Using the Calculator

Tips: Enter K_p value, initial pressure in atm, and stoichiometric coefficients separated by commas (reactants first, then products). All values must be valid (K_p > 0, pressure > 0).

5. Frequently Asked Questions (FAQ)

Q1: What's the difference between K_p and K_c?
A: K_p uses partial pressures while K_c uses concentrations. They're related by K_p = K_c(RT)^Δn.

Q2: When does K_p have units?
A: K_p has units when the sum of product coefficients differs from the sum of reactant coefficients.

Q3: How does temperature affect K_p?
A: K_p changes with temperature according to the van't Hoff equation.

Q4: Can K_p be used for liquids or solids?
A: No, K_p is only for gases. Pure liquids and solids are not included.

Q5: What if my reaction has multiple steps?
A: For multiple equilibria, the overall K_p is the product of individual K_p values.