Post a New Question

college chemistry

posted by .

For the equilibrium Br2 + Cl2 goes to 2BrCl at 400 K ,Kc = 7.0. 0.30 of Br2 and 0.30 of Cl2 are introduced into a 1.0 L- container at 400 K.a) What will be the equilibrium concentration of Br2? b) What will be the equilibrium concentration of Cl2 ? c) What will be the equilibrium concentration of BrCl?

  • college chemistry -

    0.30 WHAT of Br2 and 0.30 WHAT of Cl2 are introduced........ I suspect you meant moles and the following answer is based on that assumption.
    0.30 moles/1 L = 0.30M for (Br2) and (Cl2) initially. Set up and ICE chart.

    ............Br2 + Cl2 ==> 2BrCl
    initial...0.30M...0.30M.....0
    change......-x....-x........2x
    equil.....0.30-x..0.30-x....2x

    Substitute the equilibrium values into the Kc expression and solve for x. From that you can calculate (Br2), (Cl2) and (BrCl) at equilibrium.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

More Related Questions

Post a New Question