Chemistry, 28.02.2020 02:23 melissapulido198

Consider the equilibrium between SbCl5, SbCl3 and Cl2. SbCl5(g) -->SbCl3(g) + Cl2(g) K = 2.30×10-2 at 566 K .The reaction is allowed to reach equilibrium in a 7.40-L flask. At equilibrium, [SbCl5] = 0.333 M, [SbCl3] = 8.75×10-2 M and [Cl2] = 8.75×10-2 M.

(a) The equilibrium mixture is transferred to a 14.8-L flask. In which direction will the reaction proceed to reach equilibrium?
(b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 14.8-L flask.

[SbCl5] = M
[SbCl3] = M
[Cl2] = M

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Consider the equilibrium between SbCl5, SbCl3 and Cl2. SbCl5(g) -->SbCl3(g) + Cl2(g) K = 2.30×10-...

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