Chemistry II

posted by .

At a certain temperature, Kc = 33 for the reaction:

H2(g) + I2(g) 2HI(g)

Assume that the initial concentrations of both H2 and I2 are 6.00 x 10-3 mol/L. Find the concentration of each reactant and product at equilibrium.

  • Chemistry II -

    You need to insert the arrow to know the difference between products and reactants. You have the equation, set up an ICE chart.
    ....................H2 + I2 ==> 2HI
    ...initial........0.006..0.006...0
    change..............-x....-x.....2x
    equilibrium.....0.006-x...0.006-x...2x

    Now substitute into the Kc expression of
    Kc = 0.33 = (HI)^2/(H2)(I2)
    Solve for x and calculate each of the final concns. Post your work if you get stuck.

  • Chemistry II -

    X=1.97406×10 power of -3 .then what is the reactant and product of equilibrium .can't understand actually .

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    1) The activation energy of a certain reaction is 35.3 kJ/mol. At 20 degrees C, the rate constant is 0.0130 s^-1. At what temperature would this reaction go twice as fast?
  2. CHEMISTRY> HELP QUICK! pls

    Calculate the reaction free energy of: H2(g) + I2(g) 2HI(g) when the concentrations are 0.026 mol L-1 (H2), 0.33 mol L-1 (I2), and 1.84 mol L-1 (HI), and the temperature is 700K. For this reaction Kc= 54 at 700 K. +11.6 kJ mol-1 0 …
  3. chemistry

    For the reaction H2(g) + I2(g) ↔ 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, …
  4. chemistry

    For the reaction H2(g) + I2(g) ↔ 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, …
  5. chemistry

    At a certain temperature, the Equilibrium constant, Kc, for this reaction is 53.3. At this temperature, 0.500 mol of H2 and 0.500 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at Equilibrium?
  6. Chemistry

    At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g)+I2(g) <--> 2HI(g) Kc= 53.3 At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration …
  7. Chemistry

    At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g)+I2(g) <-> 2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration …
  8. chemistry - (Dr. Bob222)

    The rate constant for a second order reaction has the value of 2.5 x 10–3 L·mol–1·s–1. If the initial concentration of reactant is 3.5 mol·L-1, what will be the molar concentration of the reactant after 2.5 minutes?
  9. 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 …
  10. Chemistry

    A 2.00L flask was filled with 4.00 mol of HI at a certain temperature and given sufficient time to react. At equilibrium the concentration of H2 was 0.400 M. Find the equilibrium concentrations of I2 and HI and then find the Keq at …

More Similar Questions