Answer:
The atomic mass of second isotope is 112.926 amu.
Explanation:
Given data:
Average atomic mass of indium = 114.818 amu
Atomic mass of one isotope = 114.903 amu
Percentage abundance of 1st isotope = 95.70%
Mass of other isotope = ?
Solution:
First of all we will calculate the percentage abundance second isotope.
100 - 95.70% = 4.3%
percentage abundance of second isotope = 4.3%
Now we will calculate the mass if second isotope.
Average atomic mass of indium = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass) / 100
114.818 = (114.903×95.70)+(x×4.3) /100
114.818 = 10996.2171 + (x4.3) / 100
114.818×100 = 10996.2171 + (x4.3)
11481.8 - 10996.2171 = (x4.3)
485.583 = x
x = 485.583 /4.3
x = 112.926
The atomic mass of second isotope is 112.926.
