Chemistry

posted by .

the initial concentration of each component was: 0.100 M H2(g), 0.100M I2(g), and 0.050 M HI(g) . The Keq = 50.2. Calculate the concentration of each component when equilibrium has been reached. The balanced chemical equation for this reactions is: H2(g) + I2(g)  2HI(g)

  • Chemistry -

    First, calculate Q
    (HI)^2/(H2)(I2) = (0.05)^2/(O>1)^2 = 0.25 which is too small; therefore the reaction will move to the right.
    ..........H2 + I2 ==> 2HI
    initial..0.1...0.1....0.05
    change..-x....-x.....+x
    equil....0.1-x..0.1-x...0.05+x

    Set up Kc = (HI)^2/(H2)(I2)
    Solve for x, 0.1-x and 0.05+x

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    On this problem I keep getting the wrong answer. I am subtracting the initial concentration of Cl2 by the equilibrium concentration then using the difference to subtract for the rest using the mole ratios. Then i used the keq constant …
  2. Chemistry

    The equilibrium constant (Keq) is the ratio of ____ concentrations to ____ concentrations at equilibrium, with each concentration raised to a power equal to the number of ____ of that substance in the balanced chemical equation.
  3. Chemistry

    1. In an equilibrium, A + B ---> C + D; "A" & "B" are mixed in a vessel at temperature "T". The initial concentration of "A" was twice the initial concentration of "B", & after the equilibrium has reached, concentration of "C" was …
  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

    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, …
  6. chemistry

    For the reaction H2(g) + I2(g) ¡ê 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, change …
  7. Chemistry

    At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.500 M. The balanced chemical equation is N2+O2<--->2NO. If more NO is added, bringing its concentration to 0.800 M, what will the …
  8. Science (Chemistry)

    4. A Beer’s Law plot was prepared for the reaction A(aq) + B(aq) AB(aq), plotting absorption over AB(aq) concentration. The linear equation for this plot was y = 78.3x. A solution was prepared by mixing 10.0mL of 0.100M A …
  9. Chemistry

    Calculate the thiocyanate concentration at equilibrium if the irone (III) ion concentration is 0.23 M and the complex ion concentration is 0.625 M t equilibrium. Keq= 138M^-1
  10. chemistry

    Calculate the thiocyanate concentration at equilibrium if the irone (III) ion concentration is 0.23 M and the complex ion concentration is 0.625 M t equilibrium. Keq= 138M^-1

More Similar Questions