Final answer:
To find equilibrium concentrations for the given chemical reaction with Kc=4.0, we use an ICE table to set up the initial concentrations, calculate the change, and determine the equilibrium concentrations for each species. We solve for 'x' the amount of reactants that change to form the products, and then back-calculate the concentrations of A, B, and C at equilibrium.
Step-by-step explanation:
The student's question requires understanding how to calculate equilibrium concentrations for a chemical reaction with a given equilibrium constant (Kc). The reaction given is aA(g) + bB(g) ⇌ cC(g), with Kc = 4.0. To find the equilibrium concentrations of A, B, and C, we can set up an ICE (Initial, Change, Equilibrium) table, with initial concentrations of A and B at 1.0 M and C at 0 M. If x is the amount of A and B that react to reach equilibrium, then the equilibrium concentrations would be [A] = 1 - ax, [B] = 1 - bx, and [C] = cx. We then plug these into the equilibrium expression Kc = [C]c / ([A]a[B]b).
For the given reaction where a = 1, b = 1, and c = 2, and given Kc, we substitute 1 - x for [A] and [B], and 2x for [C], since no C is initially present. We would then solve for x and back-calculate [A], [B], and [C]. However, to give a definitive answer, we would need the actual values for a, b, and c applied to this specific reaction, not the placeholders.