The chemical equation shows the decomposition of ammonium nitrate open paren NH sub 4 NO sub 3 close paren 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?
First convert ammonium nitrate to moles: 160.1 g ÷ 80.03 g/mol ≈ 2.000 mol NH₄NO₃. The balanced equation shows that each mole of NH₄NO₃ produces 2 moles of H₂O, so about 4.000 mol of water form. Multiplying by water’s molar mass gives 4.000 mol × 18.01 g/mol ≈ 72.06 g, so the answer is 72.06 grams.
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