Answer to Question #263495 in General Chemistry for Melon

Question

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).

Answer 1

Use the balanced equation to write an equilibrium expression. Find the initial concentration of ICl from the given amount and container volume, use the balanced equation to define x and set up a reaction table, substitute into the equilibrium expression, and solve for x, from which the equilibrium concentrations can be calculated.

[ICl]mlt = (0.500 mol/5.00 L) = 0.100 M

x = 0.0331662 – 0.663324x

1.663324x = 0.0331662

x = 0.0199397

[I₂]eq = [Cl₂]eq = x = 0.0199397 = 0.0200 M

[ICl]eq = 0.100 – 2x = 0.100 – 2(0.0199397) = 0.0601206 = 0.060 M ICl