Nitrous oxide (N 2 O) can be produced by thermal decomposition of ammonium nitrate: NH 4 NO 3 ( s ) → heat N 2 O ( g ) + 2 H 2 O ( l ) What volume of N 2 O( g ) collected over water at a total pressure of 94.0 kPa and 22°C can be produced from thermal decomposition of 8.68 g NH 4 ,NO 3 ? The vapor pressure of water at 22°C is 21 torr.

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Interpretation Introduction Interpretation: The total pressure, temperature and mass of ammonium nitrate is given. The nitrous oxide produced by the given reaction is to be calculated. Concept introduction: The ideal gas equation is given as, Pressure × Volume = Number of moles × Gas constant × Absolute temperature To determine: The nitrous oxide produced by the given reaction. Explanation Given The mass of ammonium nitrate is 8.68 g . The total pressure is 94 kPa = 0.93 atm . The absolute temperature is 22 ∘ C + 273 = 295 K . Ammonium nitrate dissociates on heating to give nitrous oxide and water. NH 4 NO 3 ( s ) → heat N 2 O ( g ) + 2 H 2 O ( l ) Therefore, one mole of ammonium nitrate forms one mole of nitrous oxide. The molar mass of NH 4 NO 3 is, 2 × 14.0067 g / mol + 3 × 15.999 g / mol + 4 × 1.0079 g / mol = 80.042 g / mol The number of moles of ammonium nitrate is calculated by the formula, Number of moles = Mass Molar mass Substitute the value of mass and molar mass of ammonium nitrate in the above formula. Number of moles = 8.68 g 80.042 g / mol = 0.1084 mol Ammonium nitrate dissociates on heating to give nitrous oxide and water. NH 4 NO 3 ( s ) → heat N 2 O ( g ) + 2 H 2 O ( l ) One mole of ammonium nitrate forms one mole of nitrous oxide

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation: The total pressure, temperature and mass of ammonium nitrate is given. The nitrous oxide produced by the given reaction is to be calculated.

Concept introduction: The ideal gas equation is given as,

Pressure×Volume=Number of moles×Gas constant×Absolute temperature

To determine: The nitrous oxide produced by the given reaction.

Explanation of Solution

Given

The mass of ammonium nitrate is 8.68 g .

The total pressure is 94 kPa=0.93 atm .

The absolute temperature is 22 ∘C+273=295 K .

Ammonium nitrate dissociates on heating to give nitrous oxide and water.

NH4NO3 (s)→heatN2O (g)+2H2O(l)

Therefore, one mole of ammonium nitrate forms one mole of nitrous oxide.

The molar mass of NH4NO3 is,

2×14.0067 g/mol+3×15.999 g/mol+4×1.0079 g/mol=80.042 g/mol

The number of moles of ammonium nitrate is calculated by the formula,

Number of moles=MassMolar mass

Substitute the value of mass and molar mass of ammonium nitrate in the above formula.

Number of moles=8.68 g80.042 g/mol=0.1084 mol

Ammonium nitrate dissociates on heating to give nitrous oxide and water.

NH4NO3 (s)→heatN2O (g)+2H2O(l)

One mole of ammonium nitrate forms one mole of nitrous oxide

Chemistry: An Atoms First Approach

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