Some SbCl5 is allowed to dissociate into SbCl3 and Cl2 at 521 K. At equilibrium, [SbCl5] = 0.226 M, and [SbCl3] = [Cl2]
Posted: Thu Feb 17, 2022 11:14 am
Some SbCl5 is allowed to
dissociate
into SbCl3 and Cl2 at 521 K.
At equilibrium, [SbCl5]
= 0.226 M, and
[SbCl3] =
[Cl2]
= 7.51×10-2 M.
Additional SbCl3 is added so
that
[SbCl3]new = 0.120 M
and the system is allowed to once again reach equilibrium.
(a) In which direction will the reaction proceed to reach
equilibrium?
to the right or to the left
(b) What are the new concentrations of reactants and products after
the system reaches equilibrium?
dissociate
into SbCl3 and Cl2 at 521 K.
At equilibrium, [SbCl5]
= 0.226 M, and
[SbCl3] =
[Cl2]
= 7.51×10-2 M.
Additional SbCl3 is added so
that
[SbCl3]new = 0.120 M
and the system is allowed to once again reach equilibrium.
(a) In which direction will the reaction proceed to reach
equilibrium?
to the right or to the left
(b) What are the new concentrations of reactants and products after
the system reaches equilibrium?