In a certain experimental procedure, a 1.00 L flask is filled with 2.00 mol of a

Question

In a certain experimental procedure, a 1.00 L flask is filled with 2.00 mol of and 2.00 mol 448 degree C. The value of the equilibrium constant for the reaction shown below is 50.5 at that temperature What are the concentrations of all the species present in the mixture after equilibrium has been established? A certain solution is made by weighing 1.20 grams of enough water to make 250 mL of solution. Assuming that all of the is dissolved Calculate the molar concentration of Calculate the of the solution

Explanation / Answer

initial.
[H2] = 2 mol / 1 L = 2 M
[I2] = 2 mol / 1 L = 2 M

H2 (g) + I2 (g) <----> 2HI
2 2 0 (initial)
2-x 2-x 2x (at equilibrium)

Kc = [HI]^2 / {[H2][I2]}
50.5 = (2x)^2 / (2-x)^2
sqrt (50.5) = 2x/(2-x)
2x/(2-x) = 7.11
2x = 14.22 - 7.11*x
x = 1.56 M
At equilibrium,
[H2] = 2-x = 2-1.56 = 0.44 M
[I2] = 2-x = 2-1.56 = 0.44 M
[HI] = 2*x = 2*1.56 = 3.12 M

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