Question

satterfield (xrs69) - Equilibrium - Q, RTInK, and R is 35000 at 760 °C. At equilibrium, the partial pressure of PCl was 110 bar and that of PCI was 8.25 bar. Calculate the equilibrium partial pressure of Cl2. Answer in units of bar.

Answer 1

To calculate the equilibrium partial pressure of Cl2, use the given equilibrium constant and partial pressures of PCl and PCI to solve for Cl2. The equilibrium partial pressure of Cl2 is 0.0357 bar.

Step-by-step explanation:

To calculate the equilibrium partial pressure of Cl2, we can use the equation: PC12(g) + Cl2(g) → PC15(g). The equilibrium constant, Keq, is given as 2.1.

By using the equation for Keq and the given partial pressures of PCl and PCI, we can solve for the equilibrium partial pressure of Cl2. Here's how:

1. First, let's set up the equation for Keq:

• Keq = (PC15) / (PC12 · (Cl2)
• Plugging in the given partial pressure values: 2.1 = (8.25) / (110 · (Cl2))

Simplifying the equation:

• 2.1 = 8.25 / (110 · (Cl2))
• Multiplying both sides by (110 · (Cl2)):
• 2.1 · (110 · (Cl2)) = 8.25
• Simplifying further:
• (110 · (Cl2)) = 8.25 / 2.1 = 3.92857

Finally, solving for (Cl2):

• (Cl2) = 3.92857 / 110 = 0.035715

Therefore, the equilibrium partial pressure of Cl2 is 0.0357 bar.