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Consider the equilibrium between SbCl5, SbCl3 and Cl2. SbCl5(g)<--------> SbCl3(g) + Cl2(g) K = 2.36×10-2 at...

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Chemistry

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

Answer & Explanation Solved by verified expert
4.4 Ratings (834 Votes)
SbCl5g SbCl3g Cl2g K 236102 at 552 K SbCl5 0359 M M1V1M2V2 0359 M 680 L M2 136 M2 01795 M    See Answer
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