Gaseous Equilibria and Kp
This section introduces the concept of Kp, which is used for gaseous equilibria where partial pressures are more easily measured than concentrations.
Kp is expressed using partial pressures of gases instead of concentrations:
For aA(g) + bB(g) ⇌ cC(g) + dD(g), Kp = (P_C^c × P_D^d) / (P_A^a × P_B^b)
Where P_A, P_B, P_C, and P_D are the partial pressures of gases A, B, C, and D respectively.
Vocabulary: Mole fraction - The proportion of a particular gas in a mixture, calculated as (moles of gas) / (total moles of all gases).
Vocabulary: Partial pressure - The pressure exerted by a single gas in a mixture, calculated as (mole fraction) × (total pressure).
To calculate Kp:
- Determine mole fractions of gases
- Calculate partial pressures
- Substitute values into the Kp expression
Example: For N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
Given: 2.15 mol N₂, 6.75 mol H₂, 1.41 mol NH₃, total pressure 10.0 atm
Calculate mole fractions, then partial pressures, and finally Kp
Understanding Kp is crucial for analyzing gaseous equilibria and complements the use of Kc for solution-based systems.