The mass of any material will depend on two factors:
The relative density for Aluminium is 2.6995g/cm³ at room temperature.
So for every cubic cm of aluminum it will weigh 2.6995 grams.
Say for example you have 10 cubic cm of aluminum, it will weigh 26.995g.
We need to convert this figure in grams to standard units (the kilogram) so divide the 26.995 by 1000 to give us 0.026995Kg. Multiply this by the 9.81m/s for the gravity of the earth. This gives us a mass of 0.26482095 Newtons.
Obviously this figure will vary depending upon how much Aluminium you have...
To find the mass we need to multiply this weight by the
Aluminum: 26.95 g for one mole Al
Average atomic mass I think.
79.9173125
For the chemical elements the correct expression is atomic weight.This value is the weighted average mass of the natural isotopes of this element.
Each isotope of an element has a different Atomic Mass, so an average is taken of all the isotopes, but the average is weighted because the natural abundance (%) of each isotope is factored in. If hydrogen-1 is much more abundant than deuterium and tritium, then the weighted average will be closer to 1 than 2 or 3 but not a whole number. The following equation shows how percent abundance factors into the weighted average. (atomic mass A)(X% abundance) + (atomic mass B)(Y% abundance)...=(weighted average of all isotopes of the element)(100% abundance)
Atomic mass is the number of protons and neutrons in an atom.
What is weighted average atomic number
average atomis mass
Average atomic mass I think.
79.9173125
For the chemical elements the correct expression is atomic weight.This value is the weighted average mass of the natural isotopes of this element.
It is basically the "average location" of all the masses. A sort of weighted average, actually.
It is basically the "average location" of all the masses. A sort of weighted average, actually.
An Aluminum atom is 26.9815 AMU on *average*.
Each isotope of an element has a different Atomic Mass, so an average is taken of all the isotopes, but the average is weighted because the natural abundance (%) of each isotope is factored in. If hydrogen-1 is much more abundant than deuterium and tritium, then the weighted average will be closer to 1 than 2 or 3 but not a whole number. The following equation shows how percent abundance factors into the weighted average. (atomic mass A)(X% abundance) + (atomic mass B)(Y% abundance)...=(weighted average of all isotopes of the element)(100% abundance)
It is its Atomic Mass and why atomic mass is frequently not a whole number.
Atomic mass is the number of protons and neutrons in an atom.
The atomic mass given on the periodic table is a weighted average of all the isotopes, weighted by abundance of each isotope