Answered

Get the answers you've been searching for with IDNLearn.com. Our platform is designed to provide trustworthy and thorough answers to any questions you may have.

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)

Sagot :

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

We appreciate your presence here. Keep sharing knowledge and helping others find the answers they need. This community is the perfect place to learn together. IDNLearn.com is committed to providing accurate answers. Thanks for stopping by, and see you next time for more solutions.