# Problem: In an analysis of interhalogen reactivity, 0.500 mol of ICl was placed in a 5.00-L flask, where it decomposed at a high T:2ICl(g) ⥫⥬ I2(g) + Cl2(g)Calculate the equilibrium concentrations of I2, Cl2, and ICl (Kc = 0.110 at this temperature).

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###### FREE Expert Solution

When dealing with equilibrium and Kc:

Kc → equilibrium units are in molarity
Kc is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

only aqueous and gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the concentrations in the equilibrium expression

Step 1: Molarity of ICl

Molarity of ICl = 0.100 M

###### Problem Details

In an analysis of interhalogen reactivity, 0.500 mol of ICl was placed in a 5.00-L flask, where it decomposed at a high T:
2ICl(g) ⥫⥬ I2(g) + Cl2(g)
Calculate the equilibrium concentrations of I2, Cl2, and ICl (Kc = 0.110 at this temperature).