Chem II - Equilibrium

posted by .

For the reaction at 430 degree C, H2 + I2 <=> 2HI Kc = 54.3. Initially 0.714 moles of H2 and 0.984 miles of I2 and 0.886 moles of HI are placed in a 2.40 L vessel. The equilibrium concentration of H2 and I2 are _____.

Ok, I tried this by changing the moles to M by dividing the moles by 2.40 liters, and subing into the Kc formula, but I did not get any of the choices listed for the multiple choice. What am I doing wrong?

  • Chem II - Equilibrium -

    You were right to change the mols to molarity by mol/2.4 = M.
    H2 + I2 ==> 2HI
    Set up an ICE chart.
    initial:
    (H2) = 0.714/2.4 =
    (I2) = 0.984/2.4 =
    (HI) = 0.886/2.4 =

    Now do the reaction quotient =
    (HI)^2/(H2)(I2) = (0.369)^2/(0.2975)(0.410) = about 1.1 or so which means at equilibrium the reaction will have gone to the right.

    change:
    (HI)= +2y
    (H2) = -y
    (I2)= -y

    equilibrium:
    (HI) = 0.369+2y
    (H2) = 0.2975-y
    (I2) = 0.41-y

    Substitute equilibrium values into Keq and solve for y and add that back into the equilibrium set up to arrive at the final concns.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chem II

    For the reaction at 430 degree C, H2 + I2 <----->2HI. Kc = 54.3. Initially 0.714 moles of H2 and 0.984 moles of I2 and 0.886 molrd of HI are placed in a 2.40 L vessel. The equilibriuim concentration of H2 and I2 is _____. This …
  2. Chemistry

    The following reaction has an equilibrium constant of 0.020 at a given temperature. 2HI(g) I2(g) + H2(g) If you have 1.00 mol HI(g) in a 0.750-L container initially, how many moles of HI(g) will be present when the system reaches equilibrium?
  3. chemistry

    Initially, there are 33 moles of A and 0 moles of B. How many moles of A and B will be present after the system reaches equilibrium?
  4. Chemistry

    At the start of the reaction there are 0.714 mole of H2, 0.984 mole of I2, and 0.886 mole of HI in a 2.70 L reaction chamber. Calculate the concentrations of the gases at equilibrium.
  5. Chemistry

    At the start of the reaction there are 0.714 mole of H2, 0.984 mole of I2, and 0.886 mole of HI in a 2.70 L reaction chamber. Calculate the concentrations of the gases at equilibrium. The equilibrium constant is 54.3.
  6. Chemistry

    A reaction mixture of 4.0 mL of 0.002 M SCN- and 5.0 mL of 0.002 M Fe3+ is diluted to 10.0 mL with 0.1 M HNO3 to form the blood-red FeNCS2+ complex. The equilibrium molar concentration of the FeNCS2+ determined from a standardization …
  7. chemistry

    Hydrogen iodide decomposes according to the reaction 2HI(g)H2(g) + I2(g) A sealed 1.50 L container initially holds .00623 moles of H2, .00414 moles of I2, and .0244 moles of HI at 703K. When equilibrium constant is reached, the concentration …
  8. chemistry

    A reaction mixture of 4.0 mL of 0.002 M SCN- and 5.0 mL of 0.002 M Fe3+ is diluted to 10.0 mL with 0.1 M HNO3 to form the blood-red FeNCS2+ complex. The equilibrium molar concentration of the FeNCS2+ determined from a standardization …
  9. Chem equilibrium

    I don't understand part b NO(g) + O3(g) <=> NO2(g) + O2(g) (a) If 2.50 moles of NO and 3.30 moles of O3 are placed in a 5.30 L flask, what is the equilibrium concentration of O2?
  10. Chemistry

    For the reaction H2(g) + I2(g) <===> 2HI(g), Kc=54.9 at 699K. A system was charged with 2.50 moles of H2 ans 2.50 moles of I2 and 5.00 moles of HI initially in a 5.00 liter vessell. How many moles of H2 should there be present …

More Similar Questions