Home
Class 11
CHEMISTRY
Naturally occuring boron has two isotope...

Naturally occuring boron has two isotopes of masses 10 amu and 11 amu. Calculate the percentage of each isotope if the average atomic mass of boron is `10.2`.

Text Solution

Verified by Experts

Let x be the fraction of B isotope and (1-x) that of .B isotope, then, `(x)10+(1-x) 11= 10.2` Fraction of B isotope, x.=0.8 (or 80%) and fraction of IB isotope, `(1-x)=0.2 (or 20%).`
Promotional Banner

Topper's Solved these Questions

  • SOME BASIC CONCAPTS OF CHEMISTRY

    BRILLIANT PUBLICATION|Exercise LEVEL-I |55 Videos

  • SOME BASIC CONCAPTS OF CHEMISTRY

    BRILLIANT PUBLICATION|Exercise LEVEL-II|50 Videos

  • S-BLOCK ELEMENTS

    BRILLIANT PUBLICATION|Exercise LEVEL-III (Linked Comprehension Type)|9 Videos

  • SOME BASIC CONCEPTS OF CHEMISTRY

    BRILLIANT PUBLICATION|Exercise LEVEL-I|55 Videos

Similar Questions

Explore conceptually related problems

Calculate the percentage of nitrogen in NH_3 (Atomic mass of N = 14, H = 1amu)

Chlorine is a mixture of two isotopes with atomic masses 35u and 37u which are present in the ratio of 3:1. Find out the average atomic mass.

Naturally occurring boron consists of two isotopes whose atomic weights are 10.01 and 11.01. The atomic weight of natural boron is 10.81. Calculate the percentage of each isotope in natural boron.

Boron' occurs in nature in the form of two isotopes '_5^(11)B' and '_5^(10)B' in ratio of 81 and 19 respectively. Calculate its average atomic máss.

Naturally occuring chlorine is a mixture of two isotopes. In every sample of this element 75.77% of the atoms are 35Cl and 24.23% are atoms of 37Cl. The accurately measured atomic mass of 35Cl is 34.9689 u and that of 37Cl is 36.9659 u. From these data. Calculate the average atomic mass of chlorine.