The reaction system POBr3 > POBr + Br2 is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of bromine is reduced by 75%?

A. POBr will be consumed as equilibrium is established

B. The partial pressure of POBr will decrease while the partial pressure of Br2 increases as equilibrium is established.

C. POBr3 will be consumed as equilibrium is established

D. The volume will have to decrease before equilibrium can be reestablished

E. Bromine will be consumed as equilibrium is established.

C. POBr3 will be consumed as equilibrium is established .

Explanation:

When a reaction change its conditions (Concentration, temperature, volume, pressure) it is possible to predict the behavior of the reaction using Le Chatelier's principle that says that for any change in a system, this one acts in an opposing way in the responding system.

Thus, in the equilibrium:

POBr₃ ⇄ POBr + Br₂

If concentration of Br₂ decreases, the system decreases concentration of POBr₃ increasing, thus, concentration of POBr and Br₂.

A. POBr will be consumed as equilibrium is established . FALSE

B. The partial pressure of POBr will decrease while the partial pressure of Br2 increases as equilibrium is established.  FALSE

C. POBr3 will be consumed as equilibrium is established . TRUE

D. The volume will have to decrease before equilibrium can be reestablished . FALSE

E. Bromine will be consumed as equilibrium is established. FALSE

I hope it helps!