Nitrosyl chloride decomposes according to the chemical equation below. 2NOCl(g) ⇌ 2NO(g) + Cl₂(g)
A pressure of 0.320 atm of nitrosyl chloride is sealed in a flask and allowed to reach equilibrium.If 22.6% of the NOCl decomposes,what is the equilibrium constant for the reaction?

Question

Quizplus · Accepted Answer

The equilibrium constant (Kp) for the reaction can be calculated using the partial pressures of the gases at equilibrium. Given that 22.6% of NOCl decomposes, the change in pressure for NOCl is -0.320 atm * 0.226 = -0.07232 atm, leaving 0.320 atm - 0.07232 atm = 0.24768 atm of NOCl. The formation of NO and Cl2 results in an increase in pressure of 0.07232 atm for each, since the stoichiometry is 1:1 for NOCl to NO and NOCl to Cl2. Therefore, at equilibrium, the partial pressures are P_NOCl = 0.24768 atm, P_NO = 0.07232 atm, and P_Cl2 = 0.07232 atm / 2 = 0.03616 atm (since 2 moles of NOCl produce 1 mole of Cl2). The equilibrium constant Kp is given by Kp = (P_NO^2 * P_Cl2) / P_NOCl^2. Substituting the values, Kp = (0.07232^2 * 0.03616) / 0.24768^2 = 0.00308.

Nitrosyl Chloride Decomposes According to the Chemical Equation Below