4 NH4NO3 -> 8 H2O + 4 N2 + 2 O2

What will be the total volume in liters of gas produced at 720. mm Hg and 570.0°C when 2.50 g of NH4NO3 completely decomposes? Use molar masses with at least as many significant figures as the data given.

2 answers

Here is an example of a stoichiometry problem. Just follow the steps. You will need to do it three times, convert NH4NO3 each time to H2O, N2, and O2 and get a total number of moles. Then convert moles, using PV = nRT at the conditions listed, to volume. Here is the link.
http://www.jiskha.com/science/chemistry/stoichiometry.html

There is a shorter way. You CAN just do the calculation one time and use the moles from the first calculation to determine all of the others.
The easiest approach is to assume that all the gases are ideal gases, so that 4 moles of NH4NO3 produces 14 moles of gas.

so 2.5 g of NH4NO3 is 2.50/80.0 moles = 0.03125 moles

which will produce 0.03125 x 14/4 moles of gas = 0.1094 moles

which is 22.4 L x0.1094 = 2.45 L at STP

then use P1V1/T1 = P2V2/T2 to find the new total volume.

Alternatively use PV=nRT, where n=0.1094.
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