Part 1:
Each molecule of NO2, nitrogen dioxide, consists of 1 atom of N and 2 atoms of O. If you have 0.155 g. of NO2, how many molecules of NO2 do you have ?
2030000000000000000000 was the correct answer
Part 2:
How many atoms of N do you have ?
I found this answer, thank you :)
See your original post below for a note.
Part 1: To determine the number of molecules of NO2 when you have a certain mass of NO2, you need to employ a series of steps:
1. Begin by calculating the molar mass of NO2. The molar mass of nitrogen (N) is approximately 14.01 g/mol, and each oxygen (O) atom has a molar mass of around 16.00 g/mol. Since NO2 consists of one N atom and two O atoms, its molar mass is:
Molar mass of NO2 = (1 × molar mass of N) + (2 × molar mass of O)
= (1 × 14.01 g/mol) + (2 × 16.00 g/mol)
= 46.01 g/mol
2. Use the molar mass of NO2 to convert the given mass (0.155 g) to the number of moles. This is done using the formula:
Moles = Mass (g) / Molar mass (g/mol)
Substituting the given values:
Moles = 0.155 g / 46.01 g/mol ≈ 0.003370 mol
3. Every mole of a compound contains Avogadro's number (6.022 × 10^23) of molecules. So, to calculate the number of molecules of NO2, multiply the number of moles by Avogadro's number:
Number of molecules = Moles × Avogadro's number
= 0.003370 mol × 6.022 × 10^23 mol^-1
≈ 2.03 × 10^21 molecules (scientific notation)
Part 2: Now let's determine the number of nitrogen (N) atoms in the given 0.155 g of NO2 molecules.
1. In 1 molecule of NO2, there is 1 atom of nitrogen (N). So, the number of nitrogen atoms is the same as the number of NO2 molecules.
Number of nitrogen atoms = Number of molecules of NO2
≈ 2.03 × 10^21 atoms (from part 1)
Therefore, in the given 0.155 g of NO2, there are approximately 2.03 × 10^21 molecules of NO2, and hence the same number of nitrogen (N) atoms.