Please help on this question

Question

Nitrogen dioxide is used in the chamber process for manufacturing sulfuric acid. It is made by direct reaction of oxygen with nitric oxide: 2 NO(g)+O2(g)->2 NO2(g). How many liters of nitrogen dioxide will be produced by the reaction of 155L of oxygen, both gases being measured at atmospheric conditions, 24 degree C and 752 torr.

 

Please solve it with work

Answer 1

You are getting "down" votes on your questions because you aren't even attempting to do them yourself.  In this forum, you should try doing the problem and then state what issues you are having.  Then tutors will be more likely to assist.

In this problem, I'll guide you, and you should do the work.  You are given the correctly balanced equation...

2 NO(g)+O2(g)->2 NO2(g)

Two ways to approach this problem.  The long way, and the short way.

Long way: From PV = nRT solve for moles (n) of O2 in 155 L of O2. (Assume NO is not limiting). Remember to convert T to Kelvin and torr to atm and use R = 0.0821 Latm/Kmole.  Then, using stoichiometry from the balanced equation, determine moles of NO2 generated from n moles of O2.  Then convert this to volume using the same equation and the same conditions of T and P.

Short way:  From Gay-Lussac's Law of constant volume and Avogadro's Law, and the correctly balanced equation, it is clear that 155 L of O2 will produce 2x155L NO2 = 310 L of NO2 (assuming NO is not limiting).