Question

1. (18 points) Consider the balanced gas phase combustion of dinitrotoluene, DNT (C7 HG(NO2)2): 2C7H6(NO2)2(g) + 3 O2(g) ---> 14 CO(g) +4 NH3(g). The products are carbon monoxide (CO) and ammonia (NH3). A gaseous mixture of DNT and O2(g) at 80°C is placed into a previously empty rigid container. When the above reaction goes to completion at 80°C, 0.15 atm of O2(g) is still present. The partial pressure of the NH3(g) produced is 1.00 atm. Assume all gases behave ideally. (a) Determine the partial pressure of CO(g) produced, the partial pressure of O2(g) present and the partial pressure of DNT present before reaction occurs. Express answers in atmospheres. As usual, show your work/reasoning and do not assume a specific volume. Reason only with the information as supplied.) P(CO)after _ atm P(O2) before atm P(DNT)before - atm

Answer 1

Calculations are shown in attached image.

(9) Partial pressure of NH₃'s 4 mol = i Prential pressure of a mol gas = P(10)atter = tx14 = 3.5 atm P(02) before = 3 + 0.15 = oig atm 1.00 atm I atm. PCONT) before = 2 = atm (6) After addition of liquid water at 80°C * pressure of NH₃(g) will not change & New pressure = 1:00 am * Pressure of co will not change New pressure = 3.5 atm * Pressure of excess of Or will not change New pressure = 0.15 atm * Total gas pressure will change new pressure = P((0) + P(NH3) + P (0₂) + P (H₂O) = 3.5 atm & 1 atm + 0.15 atm +0.46 atm 5.11 atm = Note - vapour pressure at doc is 0.46 atm