(Ideal behavior) Consider the reaction of nitric oxide and oxygen to form nitrou
ID: 885234 • Letter: #
Question
(Ideal behavior) Consider the reaction of nitric oxide and oxygen to form nitrous oxide in a closed container. The container initially held 1.39 g of oxygen and 2.432 g of nitric oxide at a pressure of 1.256 atm and a temperature of 34.5oC. What is the pressure after the reaction if the volume and the final temperature are uncharged. Give your answer to the correct number of significant figures. The reaction to consider is 2 NO + O2 -----> 2 NO2
(We often overlook the real chemistry that will occur, what is probably the most important complication we have overlooked?)
Explanation / Answer
2 NO + O2 -----> 2 NO2
No of moles of NO = 2.432/30 = 0.0811 mole
No of moles of O2 = 1.39/32 = 0.0434 mole
initial Total moles = 0.0811+0.0434 = 0.1245 mole
volume of container = 0.1245*0.0821*(34.5+273.15)/1.256
= 2.5 L
from equation 2 mole NO = 1 mole O2
limiting reagent is NO
No of moles of NO2 produced = 0.0811 mole
No of moles of O2 unreacted = 0.0434- 0.0405 = 0.0029 mole
total no of moles after the reaction = 0.0029+0.0811 = 0.084 mole
final pressure P = 0.084*0.0821*(34.5+273.15)/2.5 = 0.84 atm
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.