The equilibrium constant, Kp, for the following reaction is 1.3x1014 at 850°c. C(s)+CO2(g)= 2 CO(g) a)Calculate the equilibrium constant, kp, for the reaction below at 850°c.
2 C(s)+2 CO2(g)= 4 CO(g)
b)Calculate the equilibrium constant, kp, for the reaction below at 850°c.
2 CO(g)= C(s)+CO2(g)
c)If the equilibrium constant, kp, is 167 for COCl2(g)= CO(g)+ Cl2(g) at 850°c, find kp for COCl2(g)=Cl2(g)+1/2 C(s) at 850°c.

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