Silver has two naturally occurring isotopes with the following isotopic masses: 47Ag 107 – 106.90509 47Ag 109 – 108.9047 The average atomic mass of silver is 107.8682 amu. The abundance of the lighter of the two isotopes is __________. 3/1

A) 0.2422B) 0.4816C) 0.5184D) 0.7578E) 0.9047

Whereby we have that in nature the amount of the lighter silver found in proportion is X and the heavier isotope of silver is present as (1-X) proportion in nature.

To calculate the relative atomic mass of silver, we have

(Mass of light weight silver)×X + (mass of heavier isotope of silver×(1-X) = relative atomic mass of silver

106.90509(X) + 108.9047(1-X)

108.9-108.9(x)+106.9(x) = 107.87

-2x-1.03 = 0.517450902926

Closest answer is c

c) .5184

The relative atomic mass of isotopes is the weighted average by the mole-fraction of abundance of these isotopes which gives the atomic weight that is listed for that element on the periodic table.

Silver has two naturally occurring isotopes with the following isotopic masses: 47Ag 107 – 106.90509 47Ag 109 – 108.9047 The average atomic mass of silver is 107.8682 amu. The abundance of the lighter of the two isotopes is __________. 3/1 A) 0.2422B) 0.4816C) 0.5184D) 0.7578E) 0.9047

Respuesta :

Otras preguntas

Silver has two naturally occurring isotopes with the following isotopic masses: 47Ag 107 – 106.90509 47Ag 109 – 108.9047 The average atomic mass of silver is 107.8682 amu. The abundance of the lighter of the two isotopes is __________. 3/1

A) 0.2422B) 0.4816C) 0.5184D) 0.7578E) 0.9047