Find the concentration of product when reactant concentration at equilibrium is given using ICE equation
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3.
H2 (g) + I2 (g) <---> 2HI (g)
At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?
Set up a table of initial and final concentrations, where the change in concentration of each reactant is designated as x.
In the reaction, the reactants are forming products. Therefore, the change would be -nx for reactants and +nx for products, where n is the stoichiometric amount.
H2(g) + I2(g) <-----> 2HI(g)
I 0.600 0.600 0
C -x -x +2x
E 0.300-x 0.300-x 2x
Kc = [HI]^2 / [I2][H2]
53.3 = (2x)^2 / (0.300-x)^2
x = ?
Plug that value back into the equilibrium for [HI].
[HI] = 2x = ?