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Container A is filled with 1 mol of BrCl undergoes decomposition to give Br₂ and Cl₂. The balanced equation is shown below:

$\text{BrCl}\left(\text{g}\right)鈬�{\text{Br}}_{\text{2}}\left(\text{g}\right){\text{+ Cl}}_{\text{2}}\left(\text{g}\right)$

Reaction quotient can be constructed by placing the concentration term of product in numerator and reactant term in denominator.

${\mathbf{Q}}_{\mathbf{C}}\mathbf{=}\frac{\left[{\mathbf{Br}}_{\mathbf{2}}\right]\left[{\mathbf{Cl}}_{\mathbf{2}}\right]}{\left[\mathbf{BrCl}\right]}$

As the reaction proceeds, there is a change in concentration until the system reaches the equilibrium. In the initial stage concentration of reactants is high and has Q value. After some time, there is a difference in concentration from its initial value. Also, there is a change in Q value. When the reaction reaches at equilibrium at a certain temperature it will equal to Q.

In container A 1 mole BrCl is converting to exactly half to its products such as Br₂ and Cl₂. Whereas container B holds 0.5 mol Br2 and Cl2 giving 1 mole BrCl. Thus, both containers filled with identical mixtures.