# When 2mol of SO2Cl2 is placed in a 2L flask at 303K 56% of the SO2Cl2 decomposes as SO2 and Cl2. What is the Kc for reaction.

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`SO_2Cl_2 <=> SO_2+Cl_2`

Mole ratio

`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`

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