decomposes to dinitrogen monoxide and water according to the following equation. NH_(4)NO_(3)(s)arrow N_(2)O(g)+2H_(2)O(l) In a certain experiment.nitrate is decomposed. Find the mass of water formed. 10.7 g 5.3g 21.4g 711.9 g Multiple Choice 10 points

To find the mass of water formed when ammonium nitrate decomposes, we need to use the balanced chemical equation and the given mass of ammonium nitrate.<br /><br />Given information:<br />- Balanced chemical equation: NH4NO3(s) → N2O(g) + 2H2O(l)<br />- Mass of ammonium nitrate (NH4NO3): 10.7 g<br /><br />Step 1: Calculate the molar mass of ammonium nitrate (NH4NO3).<br />Molar mass of NH4NO3 = 14.01 (N) + 4 × 1.01 (H) + 3 × 16.00 (O) = 80.05 g/mol<br /><br />Step 2: Calculate the number of moles of ammonium nitrate.<br />Moles of NH4NO3 = 10.7 g / 80.05 g/mol = 0.134 mol<br /><br />Step 3: Use the balanced chemical equation to find the number of moles of water (H2O) formed.<br />According to the balanced equation, 1 mole of NH4NO3 produces 2 moles of H2O.<br />Moles of H2O = 0.134 mol NH4NO3 × 2 = 0.268 mol H2O<br /><br />Step 4: Calculate the mass of water (H2O) formed.<br />Molar mass of H2O = 18.02 g/mol<br />Mass of H2O = 0.268 mol × 18.02 g/mol = 4.83 g<br /><br />Therefore, the mass of water formed when 10.7 g of ammonium nitrate decomposes is 4.83 g.<br /><br />The correct answer is 5.3 g.