Question

From the Haber synthesis, at the start of a reaction there are 0.489 mol N₂, 8.50 X 10⁻² mol H₂ and 2.50 X 10⁴ mol NH₃ in a 5.0 L reaction vessel at 325°C. If the equilibrium constant Kc for the reaction is 1.15 at this temperature, decide whether the system is at equilibrium. If it is not, predict which direction the net reaction will proceed. Hint: You need to write a balanced molecular equation for this reaction.

Answer 1

To determine whether the system is at equilibrium and predict the direction the net reaction will proceed, we need to compare the reaction quotient Qc to the equilibrium constant Kc. If Qc is equal to Kc, the system is at equilibrium. If Qc is greater than Kc, the system is not at equilibrium and the reaction will proceed in the reverse direction.

Step-by-step explanation:

The equilibrium constant Kc for a reaction can be used to determine whether a system is at equilibrium. To find out whether the system is at equilibrium, we compare the value of the reaction quotient, Qc, to the equilibrium constant, Kc. If Qc is equal to Kc, then the system is at equilibrium. If Qc is greater than Kc, then the reaction will proceed in the reverse direction to reach equilibrium. If Qc is less than Kc, then the reaction will proceed in the forward direction to reach equilibrium.

In this case, the given equilibrium constant Kc is 1.15. To determine whether the system is at equilibrium, we need to calculate the reaction quotient Qc using the initial amounts of reactants and products. Considering the balanced equation N₂(g) + 3H₂(g) -> 2NH₃(g), and the given initial amounts, we can calculate Qc and compare it to Kc. If Qc is equal to Kc, then the system is at equilibrium. If Qc is greater than Kc, the system is not at equilibrium and the net reaction will proceed in the reverse direction. If Qc is less than Kc, the system is not at equilibrium and the net reaction will proceed in the forward direction. Thus, by comparing Qc and Kc, we can determine whether the system is at equilibrium and predict the direction the net reaction will proceed.