Ask Question
12 July, 04:05

Consider the following reaction:

Br2 (g) + Cl2 (g) ⇌ 2BrCl (g), Kp=1.112 at 150 K.

A reaction mixture initially contains a Br2 partial pressure of 751 torr and a Cl2 partial pressure of 737 torr at 150 K.

Calculate the equilibrium partial pressure of BrCl.

+3
Answers (1)
  1. 12 July, 06:17
    0
    the equilibrium partial pressure of BrCl is pBC = 784.52 torr

    Explanation:

    Since

    Br₂ (g) + Cl₂ (g) ⇌ 2BrCl (g), Kp=1.112 at 150 K

    denoting BC as BrCl, B as Br₂, C as Cl₂, p as partial pressure, then

    Kp = pBC²/[pB*pC]

    solving for pBC

    pBC = √ (Kp*pB*pC)

    replacing values

    pBC = √ (Kp*pB*pC) = √ (1.112*751 torr*737 torr) = 784.52 torr

    pBC = 784.52 torr

    then the equilibrium partial pressure of BrCl is pBC = 784.52 torr
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Consider the following reaction: Br2 (g) + Cl2 (g) ⇌ 2BrCl (g), Kp=1.112 at 150 K. A reaction mixture initially contains a Br2 partial ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers