Question

At 400 K, the equilibrium constant for the reaction Br 2 (g) + Cl 2 (g) 2BrCl (g) is K p = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br 2 (g), 1.00 atm of Cl 2 (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true.

Answer 1

The reaction shifts to the right as long as the ratio of initial concentrations of products to initial concentrations of reactants is small.

Step-by-step explanation:

Hello,

Since Q is defined at the actual conditions as:

`Q=([BrCl]^2)/([Br_2][Cl_2]) \\Q=(2^2)/(1*1)\\ Q=4`

One can state that for this reaction, it shifts to the right as long as the ratio of initial concentrations of products to initial concentrations of reactants is small, thus, the reagents must be consumed to attain the equilibrium.

Best regards.