Question

What is the mass (in grams) of 4.97 x 10^24 molecules of NO2?

a. Converting number of molecules to grams
b. Calculating molecular weight of NO2
c. Determining the molar volume of NO2
d. Converting grams to molecules in NO2

Answer 1

To find the mass of 4.97 x 10^24 molecules of NO2, convert the number of molecules to moles using Avogadro's number, and then multiply by the molar mass of NO2 to get 379.5 grams.

Step-by-step explanation:

The mass of 4.97 x 1024 molecules of NO2 can be calculated by first converting the number of molecules to moles using Avogadro's number, then converting moles to grams using the molar mass of NO2.

1. First, we find the number of moles of NO2 using Avogadro's number (6.022 x 1023 molecules/mol): 4.97 x 1024 molecules / 6.022 x 1023 molecules/mol = 8.25 moles of NO2.
2. Next, we calculate the molar mass of NO2 from its molecular weight: (1 x 14.0 g/mol nitrogen) + (2 x 16.0 g/mol oxygen) = 46.0 g/mol.
3. Finally, we determine the mass of the NO2 by multiplying the number of moles by the molar mass: 8.25 moles x 46.0 g/mol = 379.5 grams of NO2.