posted by Sarah .
Nitric oxide (NO) reacts with molecular oxygen as follows:
2NO(g) + O2(g) ¨ 2NO2(g)
Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end of the reaction and calculate their partial pressures. Assume that the temperatures remains constant at 25 Celsius.
Calculate the partial pressure of NO, O2 and NO2.
Volume of NO= 4.00L
Pressure of No= 0.500atm
Pressure of O2= 1.97 atm
Volume of O2 = 1.00 L
Chemistry - DrBob222, Sunday, October 31, 2010 at 8:08pm
2NO + O2 ==> 2NO2
mols NO =?? Use PV = nRT
moles O2 = ?? Use PV = nRT
From moles determine the identity of the limiting reagent, use that determine how much of the other reagent remains unreacted, then use PV = nRT to determine pressure of the "other" reagent and pressure o the product. Post your work if you get stuck.
Chemistry - Sarah, Sunday, October 31, 2010 at 8:28pm
PNO2= 2.00 atm x L/(4.00 L + 1.97 L)= 0.335 atm
PO2= 0.97 atm x L/ (4.00 L + 1.97 L)= 0.162 atm
Show step by step how do I get PNO.
First things first.
The problem states NO is 0.5 atm and 4.00 L initially. But you haven't calculated n for NO.
The problem states O2 is 1.97 atm and 1.00 L but you have used 0.97 atm and 4.00 L. And there are other errors/typos, too. I may not be interpreting your answer correctly.
How would you calculate the problem I am confuse. Please show me.
I gave you step by step the first time.
You can substitute as well as I.