The chemical equation shows the decomposition of ammonium nitrate (NH4NO3). NH sub 4 NO sub 3 rightarrow cap n sub 2 cap o plus 2 cap h sub 2 cap o A chemist who is performing this reaction starts with 160 point 1 g of NH sub 4 NO sub 3 The molar mass of NH sub 4 NO sub 3 is 80 point 0 3 g over mol ; the molar mass of water open paren cap h sub 2 cap o close paren is 18 point 0 1 g over mol What mass, in grams, of cap h sub 2 cap o is produced?
The balanced equation shows that 1 mole of NH₄NO₃ produces 2 moles of H₂O. The starting amount is 160.1 g ÷ 80.03 g/mol ≈ 2.000 moles of NH₄NO₃, so it produces about 4.000 moles of water. Multiplying by water’s molar mass gives 4.000 mol × 18.01 g/mol ≈ 72.06 g, which is choice A.
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