The equilibrium constant of concentration (Kc) expresses the ratio of concentrations [ C ] of products over reactants for a reaction that is at equilibrium.
2 ICl rightleftharpoons "Cl_2 + I_2
The equilibrium constant is written as:
K_C = ([I_2] [Cl_2])/([ICl]^2)
"If :"
K_C>1 => "equilibrium favors Products"
K_C<1 => "equilibrium favors the Reactants"
underline"DATA"
[ICl]_0 = "0.682 g" /"162.357 (g/mol)""= 0.00420 mol"
"Molarity"-> [ICl]_0 = "0.0042 mol" /"0.765 (L)"= 0.00549 M
[I_2]_E = "0.0383 g" /"253.808(g/mol)""= 0.000151 mol"
"Molarity"-> [I_2]_E = "0.000151 mol" /"0.765 (L)"= 0.000197 M = [Cl_2]_E
underline"CONC. AT EQUILIBRIUM"
[ICl]_E = [ICl]_0 - [I_2]_E. - [Cl_2]_E = 0.00549 - 2(0.000197) =
0.005096 M
SUBSTITUTING DATA IN K_C
K_C = ([0.000197] [0.000197])/([0.005096]^2)= color(blue)0.00149