Iodine and bromine react to give iodine monobromide, IBr I2+Br2 is in equilibrium to yield 2IBr...

Iodine and bromine react to give iodine monobromide, IBr

I2+Br2 is in equilibrium to yield 2IBr

What is the equilibrium composition of a mixture at 115°C that initially contained 1.30 x 10 to the negative third 1.30 mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant Kc for this reaction at 115°C is 55.8.

I2 = M ?

Br2= M ?

IBr= M ?

Solutions

Expert Solution

I2 + Br2 ------------->2IBr

I 0.0013 1.3 0

C -x -x 2x

E 0.0013-x 1.3-x 2x

[I2] = 0.0013-x/5

[Br2] = 1.3-x/5

[IBr] = 2x/5

Kc = [IBr]^2/[Br2][I2]

55.8 = (2x)^2/(0.0013-x)(1.3-x)

55.8*(0.0013-x)(1.3-x) = 4x^2

x = 0.00129

[I2] = 0.0013-x/5 = 0.0013-0.00129/5 = 0.000002M

[Br2] = 1.3-x/5 = 1.3-0.00129/5 = 0.259M

[IBr] = 2x/5 = 2*0.00129/5 = 0.000516M

queen_honey_blossom answered 1 year ago

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