Final answer:
Changes in initial concentrations of Br2 and Cl2 will affect the equilibrium concentration of BrCl. An increase in initial concentrations of Br2 and Cl2 will increase the equilibrium concentration of BrCl and vice versa. This is a result of the reaction's attempt to re-establish equilibrium, according to Le Châtelier's principle.
Step-by-step explanation:
The question revolves around the impact of different initial concentrations of reactants (Br2 and Cl2) on the equilibrium concentration of the product, BrCl. This topic is related to the concept of Chemical Equilibrium in Chemistry. Every chemical reaction tending towards equilibrium is guided by the Le Châtelier's principle which determines the direction of shift in the reaction in response to disturbances such as concentration, temperature, volume and pressure changes.
As per Le Châtelier's principle, if the concentrations of Br2 and Cl2 are increased (disturbance), the reaction will shift in a direction to lower their concentrations, which is the forward direction of the reaction forming BrCl. Thus, an increase in the initial concentrations of Br2 and Cl2, will lead to a higher equilibrium concentration of BrCl.
Conversely, if the initial concentrations of Br2 and Cl2 are reduced, the reaction, in an effort to counter this disturbance, shifts towards the reverse direction, reducing BrCl production, and therefore resulting in a lower equilibrium concentration of BrCl. Remember that these shifts in reaction help re-establish the equilibrium and does not change the equilibrium constant (K).
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