Consider a production of ammonia reaction N₂ (g) + 3H₂ (g) ⇌ 2NH₃
Calculating the Kₚ of the Reaction
This reaction has a Kc of 9.6 at 300 °C. What is the Kₚ of this reaction?
Given information:
- Kc = 9.6
- Temperature (T) = 300 °C
Final answer:
The equilibrium constant expression, Kₚ, for the given reaction is the partial pressure of ammonia squared divided by the partial pressure of nitrogen multiplied by the partial pressure of hydrogen cubed.
Explanation:
The equilibrium constant expression for the given reaction is [NH₃]2[N₂][H₂]3. Since we are looking for the equilibrium constant expression in terms of partial pressures, we can rewrite it as (P(NH₃))2 / (P(N₂))(P(H₂))3. The equilibrium constant expression, Kₚ, is the partial pressure of ammonia squared divided by the partial pressure of nitrogen multiplied by the partial pressure of hydrogen cubed.
What is the Kₚ of the ammonia production reaction given a Kc of 9.6 at 300 °C? The Kₚ of this reaction is 19.2 (d).