The mass (in grams) of [tex]{\text{6}}{\text{.022}}\times{\text{1}}{{\text{0}}^{{\text{23}}}}\;{\text{atoms}}[/tex] of mass 16 amu is [tex]\boxed{{\text{16 g}}}[/tex] .
Further Explanation:
Avogadro’s number is number of units that are present in one mole of substance. Its value is equal to [tex]{\text{6}}{\text{.022}}\times{\text{1}}{{\text{0}}^{{\text{23}}}}\;{\text{units}}[/tex] per mole of substance. These units can be electrons, atoms, molecules or ions.
Amount of substance is measured in terms of mole. The mass of substance with same number of fundamental units as atoms in 12 g of carbon 12 is 1 mole.
AMU refers to atomic mass unit. It is defined as 1/12th of mass of a carbon-12 atom. It is used to indicate relative masses of various isotopes. For example, uranium-235 has mass 235 amu whereas its other isotope uranium-238 has mass 238 amu.
It is given that [tex]{\text{6}}{\text{.022}}\times{\text{1}}{{\text{0}}^{{\text{23}}}}\;{\text{atoms}}[/tex] has mass of 16 amu. According to the definition of Avogadro’s number, [tex]{\mathbf{6}}{\mathbf{.022 \times1}}{{\mathbf{0}}^{{\mathbf{23}}}}\;{\mathbf{atoms}}[/tex] are present in 1 mole of the substance.
This indicates the mass of one mole of the substance is 16 g.
Learn more:
1. Calculate the mass of ammonia: https://brainly.com/question/6078553
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Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Mole concept
Keywords: mole, Avogadro number, amu, carbon-12, atoms, 16 amu, 16 g, ions, molecules, 12g, amount of substance, atomic mass unit, formula units and number of units.
