Question

Consider this equilibrium reaction at 400 K. Br₂(g)+Cl₂(g) ⇿ 2BrCl(g)Kc=7.0 If the composition of the reaction mixture at 400 K is [BrCl]=0.004150 M, [Br₂]=0.003660 M, and [Cl₂]=0.0006720 M, what is the reaction quotient, ?

so = ____

Answer 1

The reaction quotient (Q) for the given reaction is approximately 7.0, which suggests that the system is at equilibrium at the provided conditions.

Step-by-step explanation:

To calculate the reaction quotient (Q) for the reaction Br₂(g) + Cl₂(g) ⇌ 2BrCl(g), we use the concentrations of the reactants and products given in the equilibrium reaction at 400 K. The reaction quotient Q is defined by the following expression, which is similar to the equilibrium constant expression but for a non-equilibrium mixture:

Q = [Products]^coefficients / [Reactants]^coefficients. For our reaction, Q is defined as: Q = [BrCl]^2 / ([Br₂] × [Cl₂]). Plugging in the values provided, we get: Q = (0.004150 M)^2 / (0.003660 M × 0.0006720 M). Q = 0.0000172225 M^2 / 0.00000245952 M^2. Q = 7.004 ≈ 7.0. Since the reaction quotient Q is approximately equal to the provided equilibrium constant Kc (7.0), the system is at equilibrium.