What mass of iron contains the same number of atoms as 70.05 g of nitrogen?
i got 3.011 x 10^24 atoms N
how do i convert this to Fe?
I see that worked for the C6H12O6 problem we worked on below. Let this be a learning experience for you. Just leave all the intermediate calculations, if possible, in the computer, and make the final rounding just once; otherwise, we get rounding errors and the more intermediate steps we use the more errors.
If you MUST copy a number down (for subtraction, addition, or something else), I usually copy MORE places (more significant figures) than I am allowed, do the math, then make a final rounding to the correct number of s.f. last.
okay thanks
i got 3.011 x 10^24 atoms N
how do i convert this to Fe?
70.05 g N2 has a molar mass of 28.01348.
70.05 x (1 mol/28.01348) x (2 atoms N/mol N2) x (6.022 x 10^23 atoms/mol) = 3.0117 x 10^24 atoms nitrogen.
1 mol Fe contains 6.022 x 10^23 atoms.
1 mol Fe has a mass of 55.847 grams.
If you're unconfortable with the factor label method, use ratio and proportion.
(Note above that I usually make a habit of using all of the numbers in a conversion, but especially here, I used 6.022 x 10^23 [instead of 6.02] because 70.05 has 4 s.f. and I wanted Avogadro's number to have 4 s.f., too.)
To determine the mass of iron that contains the same number of atoms as 70.05 g of nitrogen, you need to compare the molar masses and Avogadro's number.
1. Find the molar mass of nitrogen (N) by looking up its atomic mass on the periodic table. Nitrogen has an atomic mass of approximately 14.01 g/mol.
2. Calculate the number of moles of nitrogen (n) in 70.05 g by dividing the mass by the molar mass:
n = m/M
n = 70.05 g / 14.01 g/mol
n ≈ 4.995 mol
Note: The value is rounded to three decimal places.
3. Use Avogadro's number (6.022 x 10^23) to determine the number of nitrogen atoms (N) in 4.995 moles:
N = n * NA
N = 4.995 mol * 6.022 x 10^23 atoms/mol
N ≈ 3.011 x 10^24 atoms
Note: The value is rounded to three significant figures.
4. Now, compare the number of nitrogen atoms to the number of iron atoms (Fe). Since iron and nitrogen have different atomic masses, the ratios of their masses to the number of atoms will be different. You need to find the mass of iron (mFe) that contains the same number of atoms as 3.011 x 10^24 nitrogen atoms.
5. Divide the number of nitrogen atoms by Avogadro's number to find the number of moles of nitrogen:
nFe = N / NA
nFe = 3.011 x 10^24 atoms / 6.022 x 10^23 atoms/mol
nFe ≈ 4.997 mol
Note: The value is rounded to three decimal places.
6. Finally, calculate the mass of iron (mFe) corresponding to 4.997 moles of iron:
mFe = nFe * MFe
(where MFe represents the molar mass of iron)
Unfortunately, I don't have the specific information for the molar mass of iron in this database, but you can check the periodic table or other reliable sources to find the molar mass of iron. Once you have the molar mass of iron, multiply it by the number of moles (4.997) to determine the mass of iron containing the same number of atoms as 70.05 g of nitrogen.
Remember to use reliable sources for accurate molar mass data!
If you know how to do these you should show us and we can check the answer and/or method for you. But we don't DO the work.
First, determine the number of atoms in 70.05 g N2, then convert that to grams Fe.