Question

The equilibrium constant for the following reaction is Kc = 8.0: A(aq) ⇌ B(aq) A flask contains 400.0 mL of 1.0 M A(aq). What is [B(aq)] when the reaction reaches equilibrium?

Answer 1

To find the concentration of B at equilibrium, use the equilibrium constant expression, Kc. With the given Kc value of 8.0 and the initial concentration of A, solve for [B]. The concentration of B at equilibrium is 8.0 M.

Step-by-step explanation:

In order to find the concentration of B at equilibrium, we can use the equilibrium constant expression, Kc. For the reaction A(aq) ⇌ B(aq), the equilibrium constant is given as Kc = 8.0.

Since the initial concentration of A is 1.0 M and the volume is 400.0 mL (or 0.400 L), we can assume that the concentration of A remains constant throughout the reaction.

Using the equilibrium constant expression, we can set up the equation: Kc = [B]/[A] = 8.0. Plugging in the known values, we get [B]/1.0 M = 8.0. Solving for [B], we find that [B] = 8.0 M.