?When 2.00 mol of \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) is placed in a 2.00 - L flask at

Chapter 15, Problem 15.74

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When 2.00 mol of \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) is placed in a 2.00 - L flask at 303 K, 56 % of the \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) decomposes to \(\mathrm{SO}_{2}\) and \(\mathrm{Cl}_{2}\) :

\(\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)\)

(a) Calculate \(K_{c}\) for this reaction at this temperature.

(b) Calculate \(K_{p}\) for this reaction at 303 K.

(c) According to Le Châtelier's principle, would the percent of \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?

(d) Use the equilibrium constant you calculated above to determine the percentage of \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) that decomposes when 2.00 mol of \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) is placed in a 15.00-L vessel at 303 K.

Text Transcription:

SO2Cl2

SO2

Cl2

SO2Cl2(g) rightleftharpoons  SO2(g) + Cl2(g)

Kc

Kp