A sealed 1.0 L flask is filled with the 0.500 mol of I 2 and 0.500 mol of Br 2 .

Question

A sealed 1.0 L flask is filled with the 0.500 mol of I2 and 0.500 mol of Br2. The following equilibrium reaction is established:

At equilibrium, the flask is found to contain 0.840 mol of IBr. What s the Value of Kc for this reaction?

Please show step by step.

A sealed 1.0 L flask is filled with the 0.500 mol of I2 and 0.500 mol of Br2. The following equilibrium reaction is established: At equilibrium, the flask is found to contain 0.840 mol of IBr. What s the Value of Kc for this reaction? Please show step by step.

Explanation / Answer

Given your reaction

I2(g) + Br2(g) <------> 2Br(g)

The equilibrium conc will be

[IBr] = 0.84 mol/l
Thus
[Br2] = [I2] = 0.5 - 0.84 / 2 = 0.08 mol/l

Keq = [IBr]^2/)([I2] [Br2]) = (0.84)^2/(0.08)^2 = 110 to 3 sig figures.

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