The equilibrium constant for the following reaction is
1.29×10-2 at 600K.
If an equilibrium mixture of the three gases at
600K contains
2.34×10-2 M
COCl2(g) and
1.39×10-2 M CO, what
is the equilibrium concentration ofCl2?
___M
Kc is defined as concentration of product by concentration of reactant with each concentration term raised to power that is equal to its stoichiometric coefficient in balanced equation
pure liquid and solid do not appear in Kc
So,
Kc = [CO][Cl2]/[COCl2]
1.29*10^-2 = (1.39*10^-2)*[Cl2]/(2.34*10^-2)
[Cl2] = 2.17*10^-2 M
Answer: 2.17*10^-2 M
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