PCL5(g) -> PCl3(g) + Cl2 (g)

Kp= 23.6 at 500K

Calculate the equlibrium partial pressures of the reactants and products if the initial pressures are Ppcl5 = 0.560atm and Ppcl3 = 0.500atm.

To calculate the equilibrium partial pressures of the reactants and products, we can use the concept of the equilibrium constant (Kp) along with the given initial pressures. The equilibrium constant relates the concentrations (or in this case, partial pressures) of the reactants and products at equilibrium.

Given:
PCL5(g) -> PCl3(g) + Cl2(g)
Kp = 23.6 (at 500K)
Initial pressures:
Ppcl5 = 0.560 atm
Ppcl3 = 0.500 atm

To solve for the equilibrium partial pressures, we'll use the following steps:

Step 1: Write the balanced chemical equation:

PCL5(g) -> PCl3(g) + Cl2(g)

Step 2: Define the change in pressure (partial pressure) of each component:

Let the change be x atm for each component.

Step 3: Use the initial pressures and change in pressure to calculate the equilibrium pressures:

This can be done by applying the principles of stoichiometry and the equilibrium constant expression.

The equilibrium constant expression for the given equation is:
Kp = (Ppcl3 * Pcl2) / (Ppcl5)

Step 4: Substitute the given values into the equilibrium constant expression and solve for the unknown:

Kp = (0.500 + x) * (x) / (0.560 - x)

Step 5: Solve the quadratic equation:

Rearrange the equation and solve for x. Once you find the value of x, you can calculate the equilibrium partial pressures as follows:

Ppcl5 (at equilibrium) = 0.560 - x
Ppcl3 (at equilibrium) = 0.500 + x
Pcl2 (at equilibrium) = x

By substituting the value of x in these equations, you can calculate the equilibrium partial pressures of the reactants and products.