Question

2 attempts left Check my work Nitrous oxide can be formed by thermal decomposition of ammonium nitrate: heat N20g)+ 2 H2OG) NHANO3) What mass of ammonium nitrate is required to produce 136 L of N20 at 2850 torr and 42,0°C? x 10

Answer 1

Given volume of N₂O=V=136 L

Temperature T=42.0^oC=42+273 K=315 K

Pressure P=2850 torr=2850 torr/760 torr/1 atm (1 atm=760 torr)

R=Gas constant=0.0821 Latm/molK

Use these values in PV=nRT where n=number of moles of the gas

(2850 torr/760 torr/atm) x 136 L=n x 0.821 Latm/molK x 315 K

n=(2850 torr/760 torr/atm) x 136 L/(0.821 Latm/molK x 315)=19.72 mol

As per the balanced chemical equation, 1 mol N₂O is produced from 1 mol NH₄NO₃

So 19.72 mol N₂O is produced from 19.72 mol NH₄NO₃

Molar mass of NH₄NO₃=2xmolar mass of N+4xmolar mass of H+3xmolar mass of O=2x14 g/mol+4x1 g/mol+3x16 g/mol

=28 g/mol+4 g/mol+48 g/mol=80 g/mol

So mass of ammonium nitrate (NH₄NO₃) required to produce given amount of nitrous oxide=number of moles x molar mass

=19.72 mol x 80 g/mol=1577.6 g

=1577.6 g/mol x 10^-3 x 10³ g=1.5776 x 10³ g