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When 2mol of SO2Cl2 is placed in a 2L flask at 303K 56% of the SO2Cl2 decomposes as SO2...
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`SO_2Cl_2 <=> SO_2+Cl_2`
`SO_2Cl_2:SO_2:Cl_2 = 1:1:1`
Amount of `SO_2Cl_2` reacted `= 56/100xx2 = 1.12`
Amount of `SO_2` formed `= 1.12`
Amount of `Cl_2` formed `= 1.12`
Remaining `SO_2Cl_2 = 2-1.12 = 0.88`
Moles at equilibrium state
`SO_2Cl_2 = 0.88`
`SO_2 = 1.12`
`Cl_2 = 1.12`
`[SO_2Cl_2] = 0.88/2 = 0.44(mol)/L`
`[SO_2] = [Cl_2] = 1.12/2 = 0.56(mol)/L`
`K_c = ([SO_2][Cl_2])/[SO_2Cl_2]`
`K_c = 0.56^2/0.44 = 0.71272M`
So the `K_c` for the reaction is `0.71272(mol)/L`
Posted by jeew-m on June 20, 2013 at 6:39 PM (Answer #1)
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