Consider the following reaction:
SO2Cl2(g)⇌SO2(g)+Cl2(g)
A reaction mixture is made containing an initial [SO2Cl2] of 2.2×10−2M . At equilibrium, [Cl2]= 1.3×10−2M .

Calculate the value of the equilibrium constant (Kc).

Question

Consider the following reaction: 
SO2Cl2(g)⇌SO2(g)+Cl2(g) 
A reaction mixture is made containing an initial [SO2Cl2] of 2.2×10−2M . At equilibrium, [Cl2]= 1.3×10−2M .

Calculate the value of the equilibrium constant (Kc).

anonymous · Answer

Can you write the expression for Kc?

anonymous · Answer

Kc=[SO2][Cl2]/[SO2Cl2]

anonymous · Answer

@harbinjolene can  you solve that now or do you want help

anonymous · Answer

I still can't seem to figure it out. I don't know what the values are for the concentrations.

aaronq · Answer

make an ice table

anonymous · Answer

$$Kc= \frac{ (1.3 \times 10 ^{-2}) (1.3 \times 10^{-2}) }{ (0.9 \times 10^{-2}) }$$

anonymous · Answer

Since the molar ratio of Cl2 and SOCl2 is 1:1, you will use the equilibrium concentration as it is given. 
However, the initial concentration of SO2Cl2 is given. To find the equilibrium concentration, you must subtract (1.3 x 10^-3) from (2.2 x 10^-3).