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Question

When 2.00 mo! of SO2Cl2SO_2Cl_2 is placed in a 2.00-L fla sk at 303 K, 56% of the SO2Cl2SO_2Cl_2 decomposes to SO2SO_2 and Cl2:Cl_2: SO2Cl2(g)SO2(g)+Cl2(g)\mathrm { SO } _ { 2 } \mathrm { Cl } _ { 2 } ( g ) \rightleftharpoons \mathrm { SO } _ { 2 } ( g ) + \mathrm { Cl } _ { 2 } ( g ) According to Le Chatelier's principle, would the percent of SO2Cl2SO_2Cl_2 that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?

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According to Le Chatelier's principle, at constant temperature, increasing the volume of the gaseous equilibrium mixture causes the system to shift in the direction that increases the number of moles of gas. Hence, the percent of SO2Cl2\mathrm{SO_2Cl_2} that decomposes would increase.

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