The following masses and natural abundances: Atomic mass of a silver is a. 108.19 amu
a. 108.19 amu
Isotopes are atoms of the same element, which have the same number of protons and electrons, but a different number of neutrons, and, because of that, different masses.
The atomic mass (M) in the periodic table is a ponderation of the masses of all isotopes found in nature. Thus, it is the summation of the percent multiplied by the mass of each isotope, so:
M = 0.5184*106.90509 + 0.4846*108.90476
M = 108.19 amu
Use the atomic masses of each of the isotopes along with their percent abundances to calculate the average atomic mass
1 mole=6.022×1023 molecules.
Mass of 6.022×1023 atoms of silver (Ag)=108g (Given, atomic mass is 108g)
⸫ Mass of one atom of Silver =108 / 6.022×1023g.
=1.79×10-22g .
Here, NA is Avogadro number which is equal to 6.023×1023 6.023 × 10 23 . Hence, the mass of 2 Ag atoms is 3.586×10−22g 3.586 × 10 − 22 g .
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