Given volume of N2O=V=136 L
Temperature T=42.0oC=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
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