Consider the reaction of NO with ozone... (Ideal Gas Law)

Question

Consider the reaction of NO with ozone (a reaction present in the stratosphere that is responsible for ozone depletion): NO + O3 -> NO2 + O2 You set up an experiment in which you have two flasks separated by a valve. Each flask has a pressure of 10 millibars (or 7.50 mmHg) and a temperature of -35.0C, mimicking the conditions in the middle of the stratosphere. One flask contains 0.0200 grams of nitrogen oxide. The second flask contains ozone and has a volume of 3.00 L. You open the valve and allow the gases to react, creating nitrogen dioxide and oxygen gas. After the reaction has gone to completion, what is the total pressure inside your two-flask apparatus? Please provide your answer in mmHg. (Determine limiting reactant)

Answer 1

Lots of stuff going on here!

I made a table for the NO flask : P = 7.5mmHg, T = -35C, n = 0.02/30 moles, V = ?

O2 flask P = 7.5 mmHg, T = -35C, n = ? V = 3L

You will use PV = nRT to find V for the NO flask (make sure to have units correct for R)

You will use PV = nRT to find n for the O2 flask (make sure to have units correct for R)

Now that you have moles of each reactant you can determine the limiting reagent and the theoretical yield of the NO2 + O2. The number of moles of these produced + moles of unreacted reagent will then be used to calculate the final pressure of the system.