   Chapter 20, Problem 92CWP

Chapter
Section
Textbook Problem

# Nitrous oxide (N2O) 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 N2O(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 NH4,NO3? The vapor pressure of water at 22°C is 21 torr.

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=Numberofmoles×Gasconstant×Absolutetemperature

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

Explanation

Given

The mass of ammonium nitrate is 8.68g .

The total pressure is 94kPa=0.93atm .

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

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,

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

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

Numberofmoles=MassMolarmass

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

Numberofmoles=8.68g80.042g/mol=0.1084mol

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

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