Deriving concentrations from data In Part A, you were given the equilibrium pres

Question

Deriving concentrations from data

In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K.

Part B

The following reaction was performed in a sealed vessel at 761 C :

H2(g)+I2(g)2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=3.95M and  [I2]=2.15M. The equilibrium concentration of I2 is 0.0600 M . What is the equilibrium constant, Kc, for the reaction at this temperature?

Express your answer numerically.

Explanation / Answer

H2(g) + I2(g) 2HI(g)

Initially, [H2] = 3.95 M ; [I2] = 2.15 M ; [HI] = 0 M

Let at eqb., [H2] = (3.95-x) M ; [I2] = (2.15-x) M ; [HI] = 2x M

Now, given that, [HI] = 0.06 M

Thus, x = 0.03

Hence at eqb., [H2] = (3.95-x) M = 3.92 M; [I2] = (2.15-x) M = 2.12 M

Now, Kc = [HI]2/{[H2]*[I2]} = (0.06)2/(3.92*2.12) = 4.332*10-4

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