What is the mass (in amu and in grams) of a single atom of Carbon-12?
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1
Understand that the atomic mass unit (amu) is defined based on the carbon-12 isotope, where 1 amu is 1/12th the mass of a carbon-12 atom.
Recognize that the mass of a single carbon-12 atom is exactly 12 amu by definition.
To convert the mass from amu to grams, use the conversion factor: 1 amu = 1.66053906660 x 10^-24 grams.
Multiply the mass of the carbon-12 atom in amu by the conversion factor to find its mass in grams.
Express the mass of a single carbon-12 atom in both amu and grams.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Atomic Mass Unit (amu)
The atomic mass unit (amu) is a standard unit of mass used to express atomic and molecular weights. It is defined as one twelfth of the mass of a carbon-12 atom, which is approximately 1.66 x 10^-27 kilograms. This unit allows for easier comparison of the masses of different atoms and molecules, as they are typically very small.
Carbon-12 is one of the most common isotopes of carbon, consisting of 6 protons and 6 neutrons in its nucleus. It is used as a standard for defining the atomic mass unit because its mass is precisely 12 amu. Understanding isotopes is crucial for calculations involving atomic mass, as different isotopes of an element can have varying masses.
To convert atomic mass units (amu) to grams, one can use the conversion factor where 1 amu is equivalent to 1.66 x 10^-24 grams. This relationship is essential for expressing the mass of atoms in a more practical unit for laboratory measurements. Knowing how to perform this conversion is vital for accurately reporting atomic masses in scientific contexts.