Asked by Dani
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.
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.
Answers
Answered by
DrBob222
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.
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.
Answered by
Dr Russ
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.
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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