Final answer:
To calculate the total pressure for a 30% yield of ammonia at equilibrium, we need to set up an ICE table, use the Ke value given, and solve for the equilibrium pressures using the equilibrium constant expression for the reaction between hydrogen and nitrogen.
Step-by-step explanation:
The question involves using the equilibrium constant (Ke) for the reaction where hydrogen and nitrogen combine to form ammonia. Given a Ke of 2.18 x 10-6 atm-2 at 700 K for this reaction, we need to calculate the total pressure required to achieve a 30% yield of ammonia at equilibrium.
We can set up an ICE (Initial, Change, Equilibrium) table to find the pressures at equilibrium and apply the equilibrium constant expression for the reaction.
Nitrogen and hydrogen react in a 1:3 ratio to yield ammonia according to the equation N2 + 3 H2 → 2 NH3. At equilibrium, the reaction's quotient (Q) must equal the equilibrium constant (Ke).
The pressure of NH3 will be 30% of what it would be at complete conversion because the yield is 30%. We can substitute the expressions for the equilibrium partial pressures of the reactants and products into the equilibrium constant expression to solve for the total pressure required.
This question requires an understanding of chemical equilibrium and the manipulation of equilibrium expressions.