Answer:
PV=nRT0.988×V=76.56×0.0821×394V=2506.6 L
Step-by-step explanation:
• amount of ammonium nitrate present is m = 1.75 kg = 1750g.
• corruption of ammonium nitrate upon heating
Reaction 2NH4NO3( s) ⟶ 2N2( g) O2( g) 4H2O( g)
Molar Mass M 80 g/mol
StoichiometricCoefficient( n) 2 2 1 4
Stoichiometric Mass m = ( n × M) ( 2 × 80) g = 160 g
From the stoichiometric mass we have 160 g of ammonium nitrate produces( 2 1 4) intelligencers ie 7 moles of gas.
thus we have number of intelligencers of feasts evolved from 1750 g of ammonium nitrate equal to
n = 7/160 × 1750 moles= 76.56 moles
• Pressure of the gases are
• P = 751 mmHg = 0.988 atm
Note 1 atm = 760 mmHg.
• Temperature of the gases are
T = 121oC = 394 K
Let the volume of feasts produced be V.
From the ideal gas equation we've
PV = nRT
0.988 × V = 76.56 ×0.0821 × 394
V = 2506.6 L