Chemistry

posted by .

After 4.00 mol of C2H4(g) and 2.50 mol of Br2 (g) are placed in a sealed 1.0L container, the reaction reaches equilibrium and is written following: C2H4(g) + Br2(g) -> C2H4Br2(g) ... Calculate the equilibrium concentrations of all three substances.

  • Chemistry -

    Wouldn't you need the Keq for this reaction?

  • Chemistry -

    It doesn't give me the Keq. The information in the question is the only information I am given.

  • Chemistry -

    You can't do it without Keq.

  • Chemistry -

    You must have a graph with the equilibrium concentration of something given.

    This Q was given to me with C2H4 having an eq. concentration of 2.5 M.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chem 203

    Br2=2Br When 1.05 mol of br2 is placed in a .950L flask, 1.20% of Br2 undergoes dissociation. Calculate the equilibrium constant Kc, for this reaction. Use ICE table.
  2. chemistry

    The initial concentration for the compounds involved in the reaction displayed were determined to be [BrI(g)] = 0.3220 mol/L, [Br2(g)] = 0.3287 mol/L, [I2(g)] = 0.004086 mol/L. Calculate the value of the equilibrium constant (Kc) at …
  3. Chemistry

    Calculate the value of the equilibrium constant (Kc) for the reaction displayed if the following equilibrium concentration data were measured at 1200 K: [Br2(g)] = 0.0001151 mol/L, [Br(g)] = 0.00004423 mol/L. Br2(g) = 2Br(g)
  4. chemistry

    Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)(equilibrium arrow) 2NO (g) + Br2 (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.46 …
  5. Chemistry

    Ranking equilibrium constants from largest to smallest according to an image?
  6. chemistry

    A 0.10-mol sample of H2(g) and a 0.10-mol sample of Br2(g) are placed in a 2.0-L container. The reaction H2(g) + Br2(g) <----> 2 HBr(g) is then allowed to come to equilibrium. A 0.20 mol sample of HBr is placed into a second …
  7. Chemistry

    A sealed 1.0L flask is charged with .500mol I2 and .500mol Br2 and an equilibrium reaction esues: I2(g)+Br2(g)=2IBr(g) When the container contents achieve equilibrium, the flask contains .84 mol of IBr. What is the value of the eqilibrium …
  8. chemistry

    At a certain temperature, Keq is 4.13 x 10^-5 for the equilibrium: 2IBr(g) ↔ I2(g) + Br2(g) Assume that the equilibrium is established at the above temperature by adding only the reactant to the reaction flask. What are the concentrations …
  9. Chemistry (Equilibrium)

    At high temperature, 0.500 mol of HBR was placed in a 1.00L container where it decomposed to give the equilibrium: 2HBr <==> H2 + Br2 At equilibrium, the [Br2] is 0.0855 mol/L. What is the value of the equilibrium constant?
  10. chemistry

    For the equilibrium below at 400 K, Kc = 7.0. Br2(g) + Cl2(g) equilibrium reaction arrow 2 BrCl(g) If 0.85 mol of Br2 and 0.85 mol Cl2 are introduced into a 2.0 L-container at 400. K, what will be the equilibrium concentrations of …

More Similar Questions