The concentration equilibrium constant at 773k for the reaction
N_2 + H_2 → 2NH is 6.0 × 10^-2.
Calculate the pressure equilibrium constant.
(R=0.08321 atm dm cube K per mole)
The pressure equilibrium constant (Kp) can be calculated using the following relation:
Kp = Kc(RT)^Δn
where Kc is the concentration equilibrium constant, R is the gas constant, T is the temperature in Kelvin, and Δn is the difference in the number of moles of gaseous products and reactants.
In this case, the reaction is: N2 + H2 → 2NH3
Δn = (2-1-1) = 0
Substituting the given values:
Kp = Kc(RT)^Δn
Kp = (6.0 × 10^-2) × (0.08321 atm dm cube K^-1 mol^-1)^(0)
Kp = 6.0 × 10^-2
Therefore, the pressure equilibrium constant of the given reaction at 773 K is 6.0 × 10^-2.