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.

Question

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.

DrBob222 · Answer

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.