Question

Determine the value of kp for the following reaction if the equilibrium concentrations are as follows: p(nocl)eq = 0.22 atm, p(no)eq = 0.10 atm, p(cl2)eq = 0.11 atm. 2 nocl(g) ⇌ 2 no(g) cl2(g)

Answer 1

The equilibrium constant (Kp) for the reaction 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) given the equilibrium partial pressures is 0.0227 atm.

Step-by-step explanation:

To find the equilibrium constant (Kp) for the given chemical reaction, which is 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g), we use the equilibrium partial pressures for each compound in the reaction.

We'll apply the expression for Kp, which is Kp = P²(NO) * P(Cl₂) / P²(NOCl).

Given the equilibrium partial pressures:

• P(NOCl) = 0.22 atm,
• P(NO) = 0.10 atm, and
• P(Cl₂) = 0.11 atm,

We can substitute these values into the expression:

Kp = (0.10 atm)² * (0.11 atm) / (0.22 atm)² = 0.01 atm * 0.11 atm / 0.0484 atm = 0.0227.

Therefore, the equilibrium constant for the reaction, Kp, is 0.0227 atm.