In an analysis of interhalogen reactivity, 0.460 mol ICl was placed in a 5.55 L

Question

In an analysis of interhalogen reactivity, 0.460 mol ICl was placed in a 5.55 L flask, where it decomposed at a high temperature.

Calculate the equilibrium concentrations of I2, Cl2, and ICl. Kc = 0.110 at this temperature.
I2
M
Cl2
M
ICl
M

Please show formula and steps.

In an analysis of interhalogen reactivity, 0.460 mol ICl was placed in a 5.55 L flask, where it decomposed at a high temperature. 2ICI(g) I2(g) + Cl2(g) Calculate the equilibrium concentrations of I2, Cl2, and ICl. Kc = 0.110 at this temperature.

Explanation / Answer

Initial concentration of ICI = 0.460/5.55 = 0.08288 M


.....2 ICl...<=>...I2...+...Cl2

I....0.08288........0..........0

C.......-2a..........+a.........+a

E...0.08288-2a......a..........a


Kc = [I2][Cl2]/[ICl]^2

= a^2/(0.08288 - 2a)^2 = 0.110


a/(0.08288 - 2a) = 0.110^(1/2) = 0.33166

1.6633a = 0.027488

a = 0.01653


[I2] = a = 0.01653 M = 0.0165 M

[Cl2] = a = 0.01653 M = 0.0165 M

[ICl] = 0.08288 - 2a = 0.04982 M = 0.0498 M

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