- #1
ngu9997
- 27
- 2
Homework Statement
Sulfur dioxide gas reacts with oxygen to produce sulfur trioxide gas. Two 2 liter flasks at 25 degrees Celsius are connected by a stopcock. One flask contains 100 grams of sulfur dioxide, and the other with oxygen to a pressure of 5 atm. When the stopcock is opened the gases react until one is completely consumed. What will be the final pressure of the system after the reaction is completed.
Homework Equations
PV=nRT
The Attempt at a Solution
I started with the balanced equation: SO2 (g) + O2 (g) = SO3 (g). I then used stoichiometry to calculate the number of moles of SO2 in the first flask, and then calculated the number of moles of O2 in the second flask using PV=nRT. I'm pretty sure that this first part is right, but if not please advise me on what to do. After this is what I'm unsure of what to do. I wasn't sure if I was supposed to find the pressure of the sum of the number of moles of the two gases using PV=nRT or to subtract the smaller number of moles of O2 gas from the larger number of moles from the SO2 gas and then use PV=nRT (because the problem statement says that one gas will be completely consumed).