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Chemistry, 05.05.2020 07:33 nickname0097

When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2:
SO2Cl2(g)⇌SO2(g)+Cl2(g)
Use the equilibrium constant you calculated above to determine the percentage of SO2Cl2 that decomposes when 2.00 mol of SO2Cl2 is placed in a 18.00 −L vessel at 303 K.
I got Kc=0.712
Thanks in advance!

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When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 an...

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