Question

Titanium(IV) chloride decomposes to form titanium and chlorine, Iike this: TiCl4)Ti(s)+2 C12(g) At a certain temperature, a chemist finds that a 5.5 L reaction vessel containing a mixture of titanium(IV) chloride, titanium, and chlorine at equilibrium has the following composition: compound amount TiCl4 3.97 g 4.69 g Ti Cl2 1.62 g с Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. К x10

Answer 1

Kc is defined as concentration of product by concentration of reactant with each concentration term raised to power that is equal to its stoichiometric coefficient in balanced equation

pure liquid and solid do not appear in Kc

So, TiCl4(l) and Ti(s) will not appear in Kc expression.

So,

Kc = [Cl2]^2

Find concentration of Cl2

Molar mass of Cl2 = 70.9 g/mol

mass(Cl2)= 1.62 g

use:

number of mol of Cl2,

n = mass of Cl2/molar mass of Cl2

=(1.62 g)/(70.9 g/mol)

= 2.285*10^-2 mol

volume , V = 5.5 L

use:

Molarity,

M = number of mol / volume in L

= 2.285*10^-2/5.5

= 4.154*10^-3 M

Use:

Kc = [Cl2]^2

= (4.154*10^-3)^2

= 1.73*10^-5

Answer: 1.7*10^-5