chem 203

posted by .

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.

  • chem 203 -

    Br2 ==> 2Br
    1.05 mol/0.950 L = ?? M

    Kc = (Br)^2/(Br2)

    Initial concns:
    (Br2) = ?? M
    (Br) = 0

    chenge in concn:
    (Br) = +2x Fill in after doing equilib.
    (Br2) = ??-x Fill after doing equilib.

    equilibrium concns:
    (Br) = 0.012*2*??
    (Br2) = ??*(1-0.012)

    Substitute into Kc expression above and solve for Kc.
    Since you have asked specifically for the ICE chart, you can complete that part of the chart after determining the concns at equilibrium. Check my thinking. Check my work. Post your work if you get stuck.

  • chem 203 -

    That didn't help :(

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. 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 …
  2. 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)
  3. chem class

    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 …
  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. CHEM:

    The bond enthalpy of the Br−Cl bond is equal to ƒ¢H‹ for the reaction BrCl(g) ¨ Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br−Cl bond. Br2(l)--->Br2(g) ƒ¢H=30.91 KJ/mol Br2(g)--->2Br2(g) …
  6. chemistry:)

    The bond enthalpy of the Br–Cl bond is equal to DH° for the reaction BrCl(g)-> Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br–Cl bond. Br2(l)--->Br2(g) ÄH=30.91 KJ/mol Br2(g)--->2Br2(g) ÄH=192.9 …
  7. chemistry:)

    The bond enthalpy of the Br–Cl bond is equal to DH° for the reaction BrCl(g)-> Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br–Cl bond. Br2(l)--->Br2(g) ÄH=30.91 KJ/mol Br2(g)--->2Br2(g) ÄH=192.9 …
  8. 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 …
  9. chem

    The reaction is Br2 (g) <---> 2Br (g). It occurs at T = 1600 C. When 1.05 mol Br2 are placed in a 2 Liter flask, 2.50% of Br2 undergoes dissociation. Calculate the Kp for the reaction. Okay so i did the ICE table for this, Br2 …
  10. chm

    The equilibrium constant for the equation 2 H2(g) + CO(g) CH3OH(g) Is 19 at a certain temperature. If there are 3.11 x 10-2 moles of H2 and 5.79 x 10-3 moles of CH3OH at equilibrium in a 6.75 L flask. What is the concentration of CO?

More Similar Questions