One liter of sulfur vapor, S8(g) , at 600 ˚ C and 1.00 atm is burned in excess pure O2 to give SO2, measured at the same temperature and pressure. What mass of SO2 gas is obtained?
Don't we all love stoichiometry? The best way to start these types of problems is with a balanced equation:
Okay, now we can use the ideal gas law:
Since we have excess (unlimited) oxygen gas, we can ignore that for this problem. Let's just focus on
Now, we can use stoichiometry to find the number of moles of
Using the periodic table, we can determine that the molar mass of
Finally, using the number of moles and the molar mass, we can determine the mass of
Hope this helps!