Still, I don't understand the steps above. Could you get it a little bit easier, please?Then you can either multiply the left hand side times N/N, and since N*amu = gram, and N* atom = mole of atoms, then
16 grams / mole of oxygen atoms = 16 grams / mole of oxygen atoms.
Equivalently, multiply the right-hand side of
16 amu / oxygen atom = 16 grams / mole of oxygen atoms
times ((1/N)/(1/N)) to get
16 amu / oxygen atom =16 amu / oxygen atom
A third way, still equivalent to the other two, is to convert the mole to atoms, and divide.
Hopefully this clears things up. If not, ask some more, being more precise about your confusion.
Yes, Still I don't understand steps of how to get the mass of O atom 16g/mole to 16 amu?nomadreid said:OK, in the absence of your responding to my request to indicate what the precise difficulty is, I will start from the assumption that you do not understand the "equation" 1 atom of O = 16 amu . Perhaps one of your main problems is that you have an error when you write
"1 amu = 1/ Avogadro's number"
This is incorrect! 1 amu = 1 gram/Avogadro's Number, approximately 1.6 x 10-24 grams.
With this in mind, I replay the last option.
Write your equation more carefully (replacing "=" by "has the mass")
The mass per 1 atom of O = 16 grams/mole = 16 amu = 16*(1.6 x 10-24 grams) = 2.56 x 10-23
Convert "mole" to Avogadro's Number, and make explicit that the units involved in the mole are oxygen atoms, and you have
16 grams/(6 x 10-23 oxygen atoms) = 2.56 x 10-23 grams/ Oxygen atom
which works out.
Does this help?
Which specific step? We can’t help you if you can’t tell us what is the problem.HCverma said:I don't understand the steps above.
In the thread #2Dale said:Which specific step? We can’t help you if you can’t tell us what is the problem.
The atomic weight of O 16g/mole is converted to amu by dividing the mass in grams by Avogadro's number (6.022 x 10^23) to get the molar mass in grams per mole. Then, this molar mass is divided by the mass of one amu (1.66054 x 10^-24 grams) to get the atomic weight in amu.
The atomic weight of O 16g/mole is used as a standard because it is the most abundant isotope of oxygen and has a whole number atomic mass. This makes it a convenient reference point for comparing the atomic weights of other elements.
No, the atomic weight of O 16g/mole is not the same as the mass number of oxygen. The atomic weight takes into account the abundance of all isotopes of oxygen, while the mass number only represents the number of protons and neutrons in the most common isotope, oxygen-16.
The atomic weight of O 16g/mole is significant in chemistry because it is used to calculate the molar mass of compounds. This is important in determining the stoichiometry of chemical reactions and in performing accurate measurements and calculations in the laboratory.
The atomic weight of O 16g/mole does not directly affect the properties of oxygen. However, the atomic weight does play a role in determining the isotopic composition of oxygen and therefore can have an indirect impact on certain properties, such as boiling point and density.