A 9g sample of solid NH4Cl is heated in a 4L container to 924.4oC and decomposes according to the following equation. NH4Cl(s) -> HCl(g) + NH3(g) at equalibrium the partial pressure of NH3 (g) is 1.346 atm. Calculate the equilibrium constant for Kp for this reaction 2. Relevant equations Kp = Pproductn/Preactantn or Kc equation and Pv = nRT 3. The attempt at a solution First I used the Ideal gas equation the amount of NH3 in the system. So n = PV/RT n = (136383.45 Pa * (4 *10-3 L))/(8.3144*1197.4K) n = 5.48*10-5 This means the concentration of the NH4Cl is. n = 9/54.45 = 0.1653 0.1653 - 2(5.48*10-5) = 0.1652 I assumed then that Cl would also have this concentration. So the Kc of the reaction = ([5.48*10-5*[5.48*10-5)/0.1652 = 1.817 * 10-8 Then Kp = Kc(RT)(delta)n Kp= 1.817 * 10-8 * (8.3144*1197.4K)1 Kp = 0.00018 = 1.8*10-4 The more I look at this the more I feel there is a much easier solution, is my solution even right?