A sample of solid NH 4 NO 3 was placed inan evacuated container and then heated

Question

A sample of solid NH4NO3 was placed inan evacuated container and then heated so that it decomposedexplosively according to the following equation: NH4NO3(s) N2O(g) +2H2O(g) At equilibrium the total pressure in the container was foundto be 3.20 atm at a temperature of 500 degrees Celcius. CalculateKp for the system. A sample of solid NH4NO3 was placed inan evacuated container and then heated so that it decomposedexplosively according to the following equation: NH4NO3(s) N2O(g) +2H2O(g) At equilibrium the total pressure in the container was foundto be 3.20 atm at a temperature of 500 degrees Celcius. CalculateKp for the system.

Explanation / Answer

According to reaction, The mole fraction of the ammonium nitrate  = number of moles / total moles                                                                   = 1 / 4 = 0.25 Mole fraction of theN2O                          = 1/4   = 0.25 Mole fraction ofH2O                                 =1/2    =0.5 Therefore partial pressure of theNH4NO3    = mole fraction * total pressure                                                                       =0.25*3.20 atm                                                                       =0.8 atm Partial pressure ofN2O                                = 3.20 atm*0.25 = 0.8 atm Partial pressure of theH2O                          = 3.20 atm *0.5                                                                      =1.60 atm Therefore equaillibrium constant, Kp =(1.60)2 * (0.8) / 0.8                                                          = 2.56

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.