Consider the equilibrium between SbCl5, SbCl3 and Cl2.
SbCl5(g)<--------> SbCl3(g) + Cl2(g) K = 2.36×10-2 at 552K
The reaction is allowed to reach equilibrium in a 6.80-L flask.At equilibrium, [SbCl5] = 0.359 M, [SbCl3] = 9.20×10-2 M and [Cl2]= 9.20×10-2 M.
(a) The equilibrium mixture is transferred to a 13.6-L flask. Inwhich direction will the reaction proceed to reach equilibrium?
(b) Calculate the new equilibrium concentrations that resultwhen the equilibrium mixture is transferred to a 13.6-L flask.
[SbCl5] =______M
[SbCl3] =______M
[Cl2] =________M
