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8. For the reaction H2(g)+I2(g)„\2HI(g); [H2] = 0.95 M; [I2] = 0.78 M; [HI] = 0.27 M. Calculate the equilibrium constant K and describe the direction (forward or reverse) of the reaction. Will adding a catalyst to the reaction alter the direction of the reaction? Why? Describe two ways you could drive the reaction forward after equilibrium is achieved.

  • Chemistry - ,

    Kc = (HI)^2/(H2)(I2) = ??
    I assume the numbers given are molarities at equilibrium.
    I don't understand the "direction of the reaction) unless you mean that we look at the value of K and determine if it favors the products or the reactants. I assume that is what you meant. I get
    (.27)^2/(0.95)(0.78 = 0.0984. The small numbers means the reaction to the left is favored. Adding a catalyst does not change K.
    Two ways to drive the reaction forward.
    1. increase concn H2.
    2. increase concn I2.

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