Sulphur has a molar mass of 32.065. Carbon has a molar mass of 12.01. 32.065 / 12.01 = 2.67. So an sulphur atom is 2.67 heavier than an carbon atom.
one gram of carbon* Avogdo's number =number of atom (many atom) one atom of carbon mean carbon have a 6 electron and 12 molar mass
12.0 + (4.00000... X 1.0) = 16.0, to the justified number of significant digits.
Carbon's atomic number is 6, therefore it has 6 protons in its atoms. Mass number is the sum of protons and neutrons in the nucleus, which is 6 + 5 = 11.
I am not sure seeing as I am trying to answer that verry question at the moment. However, I believe that it would be 0% because the atomic mass you see on the periodic table is accualy an avrige of cabon 12 amu and all of its isotopes. thus the likleyhood that there is accualy a carbon particle with 12.011 is unlikely. course don't quote me on that im not entierly sure. I am not sure seeing as I am trying to answer that verry question at the moment. However, I believe that it would be 0% because the atomic mass you see on the periodic table is accualy an avrige of cabon 12 amu and all of its isotopes. thus the likleyhood that there is accualy a carbon particle with 12.011 is unlikely. course don't quote me on that im not entierly sure.
Atomic mass.
It is calculated as the ratio of the mass of one atom of an element to one twelfth of the mass of an atom of carbon-12. In fact, the weighted average of the mass of an atom of an element - weighted according to its isotopic abundance.
One atomic mass unit (amu)
The average atomic mass is the ratio of the average mass of one atom of an element to one twelfth of the mass of an atom of carbon-12. It is, the mass of an atom of the substance, rescaled so that carbon-12 would have a mass of 12.
One-twelfth the mass of a carbon-12 atom or 1,660538921(73)×10−27 kg.
It is calculated as the ratio of the mass of one atom of an element to one twelfth of the mass of an atom of carbon-12. In fact, the weighted average of the mass of an atom of an element - weighted according to its isotopic abundance.
It is calculated as the ratio of the mass of one atom of an element to one twelfth of the mass of an atom of carbon-12. In fact, the weighted average of the mass of an atom of an element - weighted according to its isotopic abundance.
It is calculated as the ratio of the mass of one atom of an element to one twelfth of the mass of an atom of carbon-12. In fact, the weighted average of the mass of an atom of an element - weighted according to its isotopic abundance.
a unit of mass used to express atomic and molecular weights, equal to one-twelfth of the mass of an atom of carbon-12. It is equal to approximately 1.66 x 10^-27 kg.
The atomic mass unit uses carbon-12 as a standard. The atomic mass unit is one twelfth of the mass of one atom of the isotope carbon-12.
One-twelfth the mass of a carbon-12 atom or 1,660538921(73)×10−27 kg.
Unified atomic mass unit, a small unit of mass used to express atomic and molecular masses. The atomic mass unit is equal to one-twelfth the mass of a carbon-12 atom or 1,660538921(73)×10−27 kg.