If a 1.60 M sample of A is heated to 500 K, what is the concentration of B at equilibrium?
A(aq)<---> 2B(aq)
Kc=9.63x10^-6
..........A --> 2B
I.......1.60.....0
C........-x......2x
E......1.60-x....2x
Assuming Kc listed is at 500K, substitute the E line into Kc expression and solve for x and 1.60-x.
To determine the concentration of B at equilibrium, we need to use the equilibrium constant expression and make use of the stoichiometry of the reaction.
The equilibrium constant expression for the given reaction is:
Kc = [B]^2 / [A]
where [B] and [A] represent the molar concentrations of B and A, respectively, at equilibrium.
Given that Kc = 9.63x10^-6, we can rewrite the equilibrium constant expression as:
9.63x10^-6 = ([B]^2) / [A]
To solve for [B], we need to know the molar concentration of A at equilibrium, which is not provided in the question. We only have the initial molar concentration of A.
Without additional information, we cannot determine the concentration of B at equilibrium.