question archive The equilibrium constant, K p , for the following reaction is 2
The equilibrium constant, K p , for the following reaction is 2
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The equilibrium constant, K p , for the following reaction is 2.01 at 500 K PCl 3 (g)+Cl 2 (g) longrightarrow PCl 5 (g) Calculate the equilibrium partial pressures of all species when PCl 3 and Cl 2 , each at an initial partial pressure 500 K introduced into an evacuated vessel at PPCl 3 = Box atm P Cl 2 = atm P PCl s = atm
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PCl3(g) + Cl2(g) --> PCl5(g)
Assume that the initial pressure is P for each PCl3 and Cl2
When the reaction reach equilibrium, assume that the partial pressure of PCl5 is x
At equilibrium,
partial pressure of PCl3 = P-x
partial pressure of Cl2 = P-x
partial pressure of PCl5 = x
Kp = [partial pressure of PCl5]/{[partial pressure of PCl3][partial pressure of Cl2]}
2.01 = (P-x)2/x
So when you has been given P or x, you are able to solve this question.
