The chemical equation below shows the decomposition of ammonium nitrate (NH4NO3).

NH4NO3 → N2O + 2H20

A chemist who is performing this reaction starts with 160.1 g of NH4NO3. The molar mass of NH4NO3 is 80.03 g/mol; the molar

mass of water (H2O) is 18.01 g/mol. What mass, in grams, of H2O is produced?

9.01

18.01

36.03

7206

72.04 g of H₂O

Explanation:

The balance chemical equation is as follow;

NH₄NO₃ → 2 H₂O + N₂O

To solve this problem we will first find the number of Moles of NH₄NO₃ as;

Moles = Mass / M. Mass

Moles = 160.1 g / 80.03 g/mol

Moles = 2.00 Moles

Secondly, we will find the number of moles of H₂O produced as,

According to equation,

1 mole of NH₄NO₃ produced = 2.0 moles of H₂O

So,

2.00 moles of NH₄NO₃ will produce = X moles of H₂O

Solving for X,

X = 2.0 moles * 2.0 mole / 1 mole

X = 4.0 moles of H₂O

Atlast, we will convert moles of water to mass as,

Moles = Mass / M. Mass

Or,

Mass = Moles * M. Mass

Mass = 4.0 mol * 18.01 g/mol

Mass = 72.04 g of H₂O