Question

Ammonium nitrate is a common ingredient in chemical fertilizers. Use the reaction shown to calculate the mass of solid ammonium nitrate that must be used to obtain 0.239 L of dinitrogen oxide gas at STP. NH4NO3(s) -> N2O(g) + 2 H2O(g)
How would you start this problem?

Answer 1

The way to start it is simply by converting 0.239 L of dinitrogen oxide gas into moles of gas using the ideal gas equation
at STP , 1 mol of gas is 22.4 L of gas, or you could simply use pv = nRT

hope this helps

Answer 2

Answer:

Mass of solid ammonium nitrate that must be used = 0.853 g

Explanation:

Given:

Volume of N2O obtained, V = 0.239 L

Temperature T at STP = 273 K

Pressure P at STP =  1 atm

Calculate the number of moles (n) of N2O obtained based on ideal gas equation:

PV = nRT

$n =\frac{PV}{RT} = \frac{1*0.239}{273*0.0821} =0.01066\ moles$

The given reaction is:

NH4NO3(s) -> N2O(g) + 2 H2O(g)

Based on the stoichiometry:

1 mole of  NH4NO3 produces 1 mole of N2O

Therefore, from the above calculation:

moles of NH4NO3 needed = 0.01066 moles

Molar mass of NH4NO3 = 80 g/mol

$Mass\ of \ NH4NO3 = moles * molar mass\\ = 0.01066\ moles * 80\ g/mol =0.8258\ g$