At 400 K, the equilibrium constant for the reaction Br₂(g) + Cl₂(g) 2BrCl (g)
Is K_p= 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br₂(g) , 1.00 atm of Cl₂(g) , and 2.00
Atm of BrCl (g) . Use Q to determine which of the statements below is true.

Question

At 400 K, the equilibrium constant for the reaction Br₂(g) + Cl₂(g)

At 400 K, the equilibrium constant for the reaction Br<sub>2 </sub>(g) + Cl<sub>2</sub><sub> </sub>(g) 2BrCl (g) Is K<sub>p </sub>= 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br<sub>2 </sub>(g) , 1.00 atm of Cl<sub>2 </sub>(g) , and 2.00 Atm of BrCl (g) . Use Q to determine which of the statements below is true. A) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. B) The equilibrium partial pressures of Br<sub>2</sub>, Cl<sub>2</sub>, and BrCl will be the same as the initial values. C) The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm. D) The reaction will go to completion since there are equal amounts of Br<sub>2</sub><sub> </sub>and Cl<sub>2</sub>. E) The equilibrium partial pressure of Br<sub>2 </sub>will be greater than 1.00 atm.

2BrCl (g)
Is K_p= 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br₂(g) , 1.00 atm of Cl₂(g) , and 2.00
Atm of BrCl (g) . Use Q to determine which of the statements below is true.

Quizplus · Accepted Answer

To determine which statement is true, we need to use the reaction quotient (Q) and compare it to the equilibrium constant (K).

The reaction quotient (Q) for this reaction is:

Q = (PBrCl)2/(PBr2 * PCl2)

Plugging in the given initial pressures we get:

Q = (2.00 atm)2/[(1.00 atm) * (1.00 atm)] = 4.00 atm

Since Q (4.00 atm) is greater than K (7.0), the reaction will shift towards the products to reach equilibrium. This means that the partial pressure of BrCl will increase, and therefore statement C is true.

Statements A, B, D, and E are all false:
A is false because the total pressure will increase due to the increase in BrCl.
B is false because the equilibrium partial pressures will be different than the initial values.
D is false because the reaction may not go to completion if equilibrium is not reached.
E is false because the equilibrium partial pressure of Br2 will decrease due to the shift towards the products.

At 400 K, the Equilibrium Constant for the Reaction Br2

At 400 K, the Equilibrium Constant for the Reaction Br₂