The molar mass of boron atoms in a natural sample is 10.71 g/mol. the sample is known to consist of 10b (molar mass 10.013 g/mol) and 11b (molar mass 11.093 g/mol). what is the percentage abundance of 11b? answer in units of %.

The percentage abundance of and 65.54 %

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:

  .....(1)

Let the fractional abundance of isotope be 'x'. So, fractional abundance of isotope will be '1 - x'

Mass of isotope = 10.013 amu

Fractional abundance of isotope = x

Mass of isotope = 11.093 amu

Fractional abundance of isotope = 1 - x

Average atomic mass of boron = 10.71 amu

Putting values in equation 1, we get:

Percentage abundance of isotope =

Percentage abundance of isotope =

Hence, the percentage abundance of and 65.54 %

at positions a, g kinetic energy is maximum.

at position d, potential energy is maximum.