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11. Calculate the atomic mass for the following isotopes of Chlorine with the following
relative abundance. (include UNITS!!!)
—Atomic Symbol
35
СІ
17
37
Cl
17
—%Natural Abundance
27.76%
72.24%

Respuesta :

Given Isotopes [tex]\sf _{17}Cl^{35},_{17}Cl^{37}[/tex]

  • Average atomic mass of Cl=35.453u

Now

Masses of isotopes are Cl-35 and Cl-37

Let

  • %abundance of Cl-35 isotope be x
  • % abundance of Cl-37 isotope =100-x

ATQ

[tex]\\ \sf\longmapsto Average\:Atomic\:Mass=\dfrac{35x+(100-x)37}{100}[/tex]

[tex]\\ \sf\longmapsto \dfrac{35x+(100-x)37}{100}=35.453[/tex]

[tex]\\ \sf\longmapsto \dfrac{35x+3700-37x}{100}=35.453[/tex]

[tex]\\ \sf\longmapsto \dfrac{-2x+3700}{100}=35.453[/tex]

[tex]\\ \sf\longmapsto -2x+3700=100(35.453)[/tex]

[tex]\\ \sf\longmapsto -2x+3700=3545.3[/tex]

[tex]\\ \sf\longmapsto -2x=3545.3-3700[/tex]

[tex]\\ \sf\longmapsto -2x=-154.7[/tex]

[tex]\\ \sf\longmapsto 2x=154.7[/tex]

[tex]\\ \sf\longmapsto x=\dfrac{154.7}{2}[/tex]

[tex]\\ \sf\longmapsto x=77.35\%[/tex]

And

[tex]\\ \sf\longmapsto 100-x=100-77.35=22.65\%[/tex]

  • %abundance of Cl-35=77.35%
  • %abundance of Cl-37=22.65%
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