Answer the following question
A(g) <--> B (g) + C(g) Kp = 2.00
Assume you placed 1.0 mole each of 'A' , 'B' , and 'C' in a container.
Without actually doing the calculations explain how you would determine whether or not the system is at equilibrium, and if not which direction would be favored to reach equilibrium.
To determine whether the system is at equilibrium or not, you need to compare the given Kp value to the calculated reaction quotient, Qp. The reaction quotient is determined by substituting the molar concentrations of the species involved in the reaction into the equilibrium expression.
In this case, the equilibrium expression is given by:
Kp = [B] * [C] / [A]
Assuming you placed 1.0 mole each of A, B, and C in the container, the initial concentration for all three species would be 1.0 M. Substituting these values into the equilibrium expression, we get:
Qp = (1.0) * (1.0) / (1.0) = 1.0
Now, compare the calculated reaction quotient (Qp = 1.0) with the given equilibrium constant (Kp = 2.00).
If Qp is less than Kp (Qp < Kp), it means there are fewer products and more reactants compared to the equilibrium position. In this case, the reaction would proceed in the forward direction to reach equilibrium.
If Qp is greater than Kp (Qp > Kp), it means there are more products and fewer reactants compared to the equilibrium position. In this case, the reaction would proceed in the reverse direction to reach equilibrium.
If Qp is equal to Kp (Qp = Kp), it means the system is already at equilibrium.
So, in this specific case, since Qp = 1.0 and Kp = 2.00, Qp is less than Kp (1.0 < 2.00). Therefore, the system is not at equilibrium, and the reaction would be favored to proceed in the forward direction to reach equilibrium.