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Answer: The atomic mass unit (referred to simply as AMU or amu) is described as 1/12 of the mass of a carbon-12 atom. The nucleus of the carbon-12 (C-12) atom includes 6 protons and 6 neutrons.
One AMU is the sum of the proton and neutron rest masses, in imprecise words.
1.67377 x 10-27 kilogramme (kg) or 1.67377 x 10-24 gramme (g). In AMU, an atom’s mass is generally equal to the nucleus’ total amount of protons and neutrons.
The AMU is used to represent and differentiate between distinct isotopes of elements by expressing their relative masses. For instance, uranium-235 (U-235) does have an AMU of roughly 235, whereas uranium-238 (U-238) has a marginally greater AMU. U-238, the most common natural isotope of uranium, contains 3 more neutrons than U-235, which has been utilized in nuclear reactors and atomic bombs.
In simpler form,
One amu = The aggregate of the proton and neutron rest masses.
1 amu is equal to 1.67377 x 10-24 grams or 1.67377 x 10-27 kilograms.
1 amu
12 amu is the mass of one atom.
1amu = (Mass of 1 126C atom divided by 12)
1amu = (1.994 x 10-23)/12
1amu = 1.662 x 10-24g.
Individual atom masses are extremely tiny. It is possible to estimate such tiny masses using a contemporary technology known as a mass spectrometer. The mass of an oxygen-16 atom, for example, is 2.66×1023g. While comparing masses measured in grams is useful, it is significantly more feasible to have a standard that allows us to evaluate comparative atomic masses more easily. The carbon-12 nuclide was chosen as the standard reference against which all additional masses were measured. One atom of carbon-12 has a mass of 12 atomic mass by definition.
