Question

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 190 bar and that of pcl3 was 9.76 bar. calculate the equilibrium partial pressure of cl2. answer in units of bar

Answer 1

The equilibrium constant (K) for the reaction PCl3(g) + Cl2(g) ⇌ PCl5(g) at 760 °C is 35000. Given the equilibrium partial pressures of PCl5 and PCl3, we can calculate the equilibrium partial pressure of Cl2 using the equilibrium constant expression. The equilibrium partial pressure of Cl2 is approximately 0.000546 bar.

Step-by-step explanation:

The equilibrium constant (K) for a reaction is a measure of the ratio of the concentrations (or pressures) of products to reactants at equilibrium. In this case, the equilibrium constant (K) for the reaction PCl3(g) + Cl2(g) ⇌ PCl5(g) is given as 35000 at 760 °C.

Given the equilibrium partial pressures of PCl5 and PCl3, we can use the equilibrium constant expression to determine the equilibrium partial pressure of Cl2. The equilibrium constant expression for this reaction is:

K = (PCl5)/(PCl3 * Cl2)

From the given data, we have PCl5 = 190 bar and PCl3 = 9.76 bar.

Substituting these values into the equilibrium constant expression:

K = (190 bar)/((9.76 bar) * Cl2)

Simplifying, we find:

35000 = (190 bar)/((9.76 bar) * Cl2)

Multiplying both sides by ((9.76 bar) * Cl2), we get:

(9.76 bar) * Cl2 = (190 bar)/35000

Dividing both sides by (9.76 bar), we find:

Cl2 = (190 bar)/((9.76 bar) * 35000)

Calculating this value, we find that the equilibrium partial pressure of Cl2 is approximately 0.000546 bar.

Answer 2

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