Final answer:
The mass of NO2 formed from 7.20×10^24 molecules of NO2 is 549.7 grams, based on the molar mass of NO2 (46 g/mol) and using Avogadro's number for the mole conversion.
Step-by-step explanation:
To calculate the mass of NO2 formed when you have 7.20×1024 molecules of NO2, we can use Avogadro's number (6.022×1023 molecules/mol), which tells us the number of molecules in one mole of a substance.
First, we need to find the number of moles of NO2, and then we can calculate its mass using the molar mass of NO2.
Number of moles = Number of molecules / Avogadro's number = 7.20×1024 molecules / 6.022×1023 molecules/mol
= 11.95 moles of NO2
The molar mass of NO2 is calculated by adding the molar masses of nitrogen (N, 14 g/mol) and oxygen (O, 16 g/mol per atom), giving us: M(NO2) = 14 + (2×16)
= 46 g/mol.
Therefore, the mass of NO2 is: Mass = Number of moles × Molar mass = 11.95 moles × 46 g/mol
= 549.7 grams of NO2.