Q) 200 L of NH3 and 120L of O2 are placed in an autoclave at 250C and 800atm. The reaction is allowed to go to completion. Determin the quantity, in moles, of the gas that remains unreacted.
A)
NH3 + (7/4) O2 ---> NO2 + (3/2) H2O
using the idea gas law I learn that
NH3 = 3723.277 moles
and
O2 = 2235.766 moles
Now (7/4)O2 = 1.75 O2
and
2235.766 / 1.75 = 1277.58
sooooooo the equation setup to represent moles looks like this
NH3 + (7/4) O2 ---> NO2 + (3/2) H2O
1277.6 + 1.75X1277.6 ---> 1277.6 + 1.5X1277.6
2235.8 1916.4
So because a greater amount of moles is shown for O2 we assume that all the oxygen was used up but we know that there were a greater number of moles for NH3
So
3726.277 - 1277.58 = 2448.7 moles unreacted.
Now Im certain this is correct, but my book course lessons show me NOTHING along these lines, is it possible to have answered this question another way??