Given the equilibrium system PCL55(g) <---> PCL3(g) + Cl2(g)
k = 12.5 at 60 degrees Celsius. A 1.0-L reaction vessel is analyzed and found to contain 3.2 mol Cl2(g), 1.5 mol PCl3(g) and 2.0 mol PCl5(g). Show that the reaction mixture has not yet reached equilibrium.
This is done the same way as the previous problem. Post your work if you get stuck and explain exactly what you don't understand about the next step.
To determine whether the reaction mixture has reached equilibrium, we need to calculate the reaction quotient, Qc, and compare it to the equilibrium constant, Kc.
The reaction quotient, Qc, is calculated by writing an expression for Qc using the molar concentrations of the reactants and products.
Qc = [PCl3] * [Cl2] / [PCl5]
Given that the reaction vessel contains 3.2 mol Cl2, 1.5 mol PCl3, and 2.0 mol PCl5, we can substitute these values into the expression for Qc.
Qc = (1.5 mol) * (3.2 mol) / (2.0 mol)
= 2.4
Now, we can compare Qc to the equilibrium constant, Kc.
Given that Kc = 12.5, and Qc = 2.4, we see that Qc is less than Kc.
Since Qc is less than Kc, it means that the reaction mixture is not at equilibrium and has not yet reached equilibrium.