The equilibrium constant for the reaction
PCl3(g) + Cl2(g)<-> PCl5(g)
is 35000 at 760◦C. At equilibrium, the partial pressure of PCl5 was 110 bar and that of PCl3 was 9.98 bar. Calculate the equilibrium partial pressure of Cl2.
Answer in units of bar
See your SO2 problem.
To solve this problem, we'll use the equation for the equilibrium constant and the partial pressure of the reactants and products.
The equilibrium constant expression for the given reaction is:
K = (P_PCl5 * P_Cl2)/(P_PCl3)
Where K is the equilibrium constant and P is the partial pressure of each substance.
We are given the value of K as 35000 and the partial pressure of PCl5 as 110 bar and PCl3 as 9.98 bar.
Substituting these values into the equation, we have:
35000 = (110 * P_Cl2)/(9.98)
To find the value of P_Cl2, we can rearrange the equation:
P_Cl2 = (35000 * 9.98) / 110
P_Cl2 ≈ 3163.18
Therefore, the equilibrium partial pressure of Cl2 is approximately 3163.18 bar.