Chemistry

posted by .

For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2] = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. If 0.340 mol of F2 is added to this equilibrium mixture, calculate the concentrations of all gases once equilibrium is reestablished.
H2(g) + F2(g) 2 HF(g)

  • Chemistry -

    You have two problems here.
    First, write Kc expression, substitute eq concns, and calculate Kc.

    Then you can address the second half of the problem.Note:I have omitted all of th zeros to save space but you should include them.
    ..............H2+ F2 ==> 2HF
    initial....0.05M.0.01M...0.400
    add..............(0.340 mol/5L = ?)
    change........-x..-x......+2x
    eqil.....0.05-x..0.078-x...0.400+2x

    Substitute the equil concns into the Kc expression and solve for x. Then plug x into the eq conditions of the ICE chart above and solve for the individual concns of each element/compound.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    Consider the balanced equation 2A(g) + 3G(g) „\ 2X(g) + Z(g). To a 20.0 L container maintained at a temperature of 127 C were added 0.200 mol of A, 0.500 mol of G, 0.400 mol of X, and 0.600 mol of Z. After equilibrium was established, …
  2. chemistry

    For the following reaction at a certain temperature, it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2] = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. If 0.261 mol of F2 is added to this equilibrium …
  3. Chemistry

    When 0.59 mol I2(g) and 0.59 mol H2(g) are placed into a 1.0-L container at a given temperature, 0.30 mol H2(g) is found to be present after the reaction below reaches equilibrium. Calculate Kc at the given temperature. I2(g) + H2(g) …
  4. Chemistry

    At a particular temperature, 13.7 mol of SO3 is placed into a 3.9-L rigid container, and the SO3 dissociates by the reaction given below. 2 SO3(g) 2 SO2(g) + O2(g) At equilibrium, 3.8 mol of SO2 is present. Calculate K for this reaction.
  5. chemistry

    please help and explain. At a certain temperature, Keq = 10.5 for the equilibrium below. CO(g) + 2 H2(g) equilibrium reaction arrow CH3OH(g) Calculate the following concentrations. (b) [H2] in an equilibrium mixture containing 1.01 …
  6. Chemistry

    For the following reaction at a certain temperature: 2( ) 2( ) ( ) 2 H F HF g g g +  it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2]=0.0500 M, [F2]=0.0100 M, and [HF]=0.400 M. If 0.200 mol F2 is …
  7. Chemistry

    Consider the equilibrium 2NOCl (g) <---> 2NO (g) + Cl2 (g). In a 1 L container @ equilibrium there are 1.0 mol NOCL, 0.70 mol NO, and 0.40 mol Cl2. @ constant temperature and volume, 0.10 mol NaCl is added. What are the concentrations …
  8. chemistry

    For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 4.87-L rigid container are [H2] = 0.0496 M [F2] = 0.0116 M [HF] = 0.429 M. H2(g) + F2(g) <==> 2 HF(g) If 0.185 mol of F2 is …
  9. chemistry

    A mixture of 0.100 mol NO, 0.200 mol H2 and 0.0800 mol N2 were placed in a 2.00L reaction vessel, heated, and allowed to come to equilibrium conditions. At equilibrium, the molar concentration of N2 was 0.0500 mol/L. Calculate Kc for …
  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