Airbags operate through the explosive reaction of sodium azide to form nitrogen gas: 20 NaN3(s) + 6 SiO2(s) +4 KNO3(s) — 32 N2(g) + 5 Na4 SiO4(s) + K4 SiO4(s) How many grams of NaN3 are required to fill an airbag with a volume of 3.00 x 104 cm3 at 75 °F and 1.00 atm of pressure?​

Under what conditions will a gas be most likely to exhibit the ideal gas properties predicted by the ideal gas law? 1)high pressures and high temperature, because particles are forced closer together with higher kinetic energy, so intermolecular forces of attraction are weaker 2)high pressure and low temperature, because particles are forced closer together and moving slower, so the volume of the particles is less significant 3) low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker 4)low pressure and low temperature, because particles are spread farther apart with lower kinetic energy, so the volume of the particles is less significant