Final answer:
To find the equilibrium pressure of Cl₂ for the given chemical reaction, we set up an ICE table, apply the equilibrium constant expression, and solve for x, which represents the change in pressure of Cl₂.
Step-by-step explanation:
To calculate the equilibrium pressure of Cl₂(g) for the reaction PCl₅(g) ⇌ PCl₃(g) + Cl₂(g), with a given Kp = 1.45 × 10⁻⁴ at 160 °C, we will use an ICE table (Initial, Change, Equilibrium). Let's set up the table with the initial pressures and the changes that occur as the system reaches equilibrium.
At equilibrium, the pressures will be:
Now, we apply the equilibrium expression using the pressure of the gases at equilibrium:
Kp = (P_PCl₃ * P_Cl₂) / P_PCl₅ = (x * x) / (3.75 - x)
Substitute the value of Kp:
1.45 × 10⁻⁴ = (x²) / (3.75 - x)
Solve this quadratic equation for x to find the equilibrium pressure of Cl₂. Note that in most cases, the x value (representing the change in pressure) will be much smaller than the initial pressure, therefore the assumption x << 3.75 can often be made to simplify calculations.