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

the answer would be b i believe