Question

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

Answer 1

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.

Answer 2

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

PNO=????

Show step by step how do I get PNO.

Answer 3

The answer is 0