Final answer:
The equilibrium partial pressure of H2 in the reaction N2 + 3H2 = 2NH3 with Keq of 13.7, given the [N2] of 1.88 M and [NH3] of 6.62 M, is 1.19 atm if ideal gas conditions apply.
Step-by-step explanation:
The task involves calculating the equilibrium partial pressure of H₂ based on the reaction N₂(g) + 3H₂(g) = 2NH₃(g) with a given equilibrium constant (Keq) at a certain temperature. Given the equilibrium concentrations of N₂ and NH₃, one needs to apply the equilibrium constant expression to find the equilibrium concentration of H₂. The expression for Keq for this reaction is Keq = ([NH₃]²)/([N₂][H₂]³).
Substituting the known values, we have:13.7 = (6.62²) / (1.88[H₂]³). Rearranging this equation to solve for [H₂]³ and then taking the cube root, we find the equilibrium concentration of H₂ to be 1.19 M.
Solving for the equilibrium partial pressure involves calculating the product of the concentration and the universal gas constant (R) multiplied by the temperature (in Kelvins). Given that the question did not provide any specifics about temperature or whether to use concentration or partial pressures, we can assume that the equilibrium partial pressure of H₂ is also 1.19 atm, assuming ideal gas conditions hold.