Question

Volume → Mass Problems (L of A → mols A → mols B → g of B)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 0.500 L of dinitrogen monoxide gas at STP. NH4NO3(s) ⇨ N2O(g) + 2H2O(g)

Answer 1

Step-by-step explanation

Given

NH4NO3(s) ⇨ N2O(g) + 2H2O(g)

Volume of N2O = 0.500 L

At STP: Temperature = 273 K

Pressure = 1 atm

Solution

Step 1: Find the moles of N2O

PV = nRT where P is the pressure, V is the volume, n is the moles, R is the gas constant (0.0821 L.atm/mol.K) and T is the tempoerature

n = PV/RT

n = (1 atm x 0.500 L)/(0.0821 L.atm/mol.k x 273 K)

n = 0.0223 mol

Step 2: Find the moles of NH4NO3

The molar ratio of NH4NO3 and N2O is 1: 1

Thereofore the moles of NH4NO3 = 0.0223 mol

Step 3: Find the mass of NH4NO3

n = m/M where n is the moles, m is the mass and M is the molar mass

m = n x M

m = 0.0223 mol x 80,043 g/mol

m = 1.78 g

Answer

Mass of NH4NO3 = 1.78 g