Respuesta :
Answer :
The abundance of [tex]^{25}\textrm{Mg}[/tex] isotope is, 10.2 %
The abundance of [tex]^{26}\textrm{Mg}[/tex] isotope is, 10.9 %
Explanation :
Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.
Formula used to calculate average atomic mass follows:
[tex]\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i[/tex] .....(1)
Let the fractional abundance of [tex]^{25}\textrm{Mg}[/tex] isotope be 'x' and the fractional abundance of [tex]^{26}\textrm{Mg}[/tex] isotope will be 'y'
For [tex]^{24}\textrm{Mg}[/tex] isotope:
Mass of [tex]^{24}\textrm{Mg}[/tex] isotope = 23.9850 amu
Fractional abundance of [tex]^{24}\textrm{Mg}[/tex] isotope = 78.99 % = 0.78899
For [tex]^{25}\textrm{Mg}[/tex] isotope:
Mass of [tex]^{25}\textrm{Mg}[/tex] isotope = 24.9858 amu
Fractional abundance of [tex]^{25}\textrm{Mg}[/tex] isotope = x
For [tex]^{26}\textrm{Mg}[/tex] isotope:
Mass of [tex]^{26}\textrm{Mg}[/tex] isotope = 25.9826 amu
Fractional abundance of [tex]^{26}\textrm{Mg}[/tex] isotope = y
Average atomic mass of magnesium = 24.3050 amu
Putting values in equation 1, we get:
[tex]24.3050=[(23.9850\times 0.78899)+(24.9858\times x)+(25.9826\times y)][/tex] .............(1)
and,
[tex]0.78899+x+y=1.00[/tex] .............(2)
or,
[tex]y=1.00-0.78899-x[/tex]
[tex]y=0.21101-x[/tex] ............(3)
Putting equation 3 in 1, we get:[tex]24.3050=[(23.9850\times 0.78899)+(24.9858\times x)+(25.9826\times (0.21101-x))][/tex]
By solving the term, we get the value of 'x'.
[tex]x=0.101839[/tex]
Now put the value of 'x' in equation 3, we get the value of 'y'.
[tex]y=0.21101-x[/tex]
[tex]y=0.21101-0.101839[/tex]
[tex]y=0.109171[/tex]
Fractional abundance of [tex]^{25}\textrm{Mg}[/tex] isotope = x = 0.101839 × 100 = 10.2 %
Fractional abundance of [tex]^{26}\textrm{Mg}[/tex] isotope = y = 0.109171 × 100 = 10.9 %