posted by alia on .
(CH3)N2H2(l) + 2N204(g) = 3N2(g) + 4H2O(l) + 2CO2(g).
consider the reaction b2n 150g of liquid (CH3)N2H2 & 80L of N2O4 at 27 degree celcius & a pressure of 2 atm. The gases produced are collected at 27 degree celsius in an evacuated 250L. Calculate:
a) Partial pressure of nitrogen produced.
You need to do the following:
1. Convert 80L N2O4 at the conditions listed to moles. Use PV = nRT and solve for n.
2. Use stoichiometry to determine the moles N2 produced. Here is an example problem, worked, that shows how to do stoichiometry.
3. Use PV = nRT to convert moles N2O4 at whatever conditions you wish (which the problem doesn't make clear) and solve for P.
By the way, note the correct spelling of celsius.