Question

An evacuated reaction vessel is filled with 3.60 atm of NOCl. When the system reaches equilibrium according to the reaction below, there are 0.160 atm of NOCl. What is Kp for this reaction? 2 NO (g) + Cl₂ (g) ⇌ 2 NOCl (g)

Answer 1

To find Kp for the reaction 2 NO (g) + Cl₂ (g) ⇌ 2 NOCl (g), we can use the equilibrium partial pressures. Given the initial pressure of NOCl and the pressure at equilibrium, we can calculate the change in pressure for NOCl and NO. Using these values, we can then calculate Kp.

Step-by-step explanation:

To find Kp for the reaction, we need to use the equilibrium partial pressures of the reactants and products. In this case, the reaction is 2 NO (g) + Cl₂ (g) ⇌ 2 NOCl (g). Given that the initial pressure of NOCl is 3.60 atm and the pressure at equilibrium is 0.160 atm, we can calculate the change in pressure for NOCl (∆P(NOCl)) as 3.60 atm - 0.160 atm = 3.44 atm. Since the stoichiometric coefficient of NOCl is 2, the change in pressure for NO (ΔP(NO)) is 2 * ∆P(NOCl) = 2 * 3.44 atm = 6.88 atm.

Finally, we can use these values to calculate Kp using the equation Kp = (∆P(NOCl))² / (∆P(NO))² = (3.44 atm)² / (6.88 atm)² = 0.81.