Question

What is the pressure of BrCl in an equilibrium mixture of Cl2, Br2, and BrCl if the pressure of Cl2 in the mixture is 0.115 atm and the pressure of Br2 in the mixture is 0.450 atm?

a) 0.565 atm
b) 0.335 atm
c) 0.450 atm
d) 0.115 atm

Answer 1

The pressure of BrCl in the equilibrium mixture is approximately 0.335 atm.

Step-by-step explanation:

To determine the pressure of BrCl in the equilibrium mixture, we can use the equilibrium constant expression (Kp) for the reaction:

Cl₂(g) + Br₂(g) = 2BrCl(g)

Kp = (P[BrCl]²) / (P[Cl₂] * P[Br₂])

Substituting the given pressures:

Kp = (P[BrCl]²) / (0.115 atm * 0.450 atm)

We can rearrange the equation to solve for P[BrCl]:

P[BrCl]² = Kp * (P[Cl₂] * P[Br₂])

P[BrCl] = sqrt(Kp * (P[Cl₂] * P[Br₂]))

Plugging in the values:

P[BrCl] = sqrt(4.7 × 10⁻² * (0.115 atm * 0.450 atm))

P[BrCl] ≈ 0.335 atm