Home
Class 11
CHEMISTRY
Nuturally occurring boron consists of ...

Nuturally occurring boron consists of two isotopes whese atomic weight are `10.01` and `11.01`The atomic weight of nurons is `10.81` Calculate the percentage of each isotope is natural boron

Text Solution

Verified by Experts

Let the percentage of isotope with atomic weight `10.01` be x .
So the percentage of isotope with atomic weight `11.01` will be `100 - x`.
Average atomic weight = `(m_(1)x_(1) + m_(2) x_(2))/(s_(1) + s_(2))`
`= (s xx 10.01 + (100 - s) xx 11.01)/(100)`
`10.81 = (s xx 10.01 + (100 - s) xx 11.01)/(100) = 20`
`%` of isotope with atomic weight `10.01 = 20`
`%` of isotope with atomic weight `11.01 = 100 - x = 80`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • ATOMIC STRUCTURE

    CENGAGE CHEMISTRY|Exercise Exercises (Subjective)|52 Videos

  • ATOMIC STRUCTURE

    CENGAGE CHEMISTRY|Exercise Exercises Linked Comprehension|50 Videos

  • APPENDIX - INORGANIC VOLUME 1

    CENGAGE CHEMISTRY|Exercise chapter-7 Single correct answer|1 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY|Exercise Archives Subjective|15 Videos

Similar Questions

Explore conceptually related problems

Naturally occureing boron consists of two insotopes whose atomic weight are 10.01 and 11.01 The atomic weight of the natural boron is 10.81 Calkculate the precentage of e ach isotopes in natURAL BORON

Naturally occurring Boron consists of two isotopes whose atomic masess are 10.01 and 11.01. The atomic mass of natural Boron is 10.81. Calculate the percentage of each isotope in natural Boron.

Knowledge Check

  • boron has two isotopes B-10,B-11. The average atomic mass of boron is found to be 10.80u. Calculate the percentage abundance of B^(10) isotope :-

    A
    80
    B
    20
    C
    25
    D
    75

  • Atomic weight of chlorine is 35.5 . It has two isotopes of atomic weight 35 and 37 . What is the percentage of the heavier isotope in the sample ?

    A
    5
    B
    10
    C
    25
    D
    20

  • Neon has two isotpoes Ne^(20) and Ne^(22) . If atomic weight of Neon is 20.2, the ratio of the relative abundances of the isotopes is

    A
    `1:9`
    B
    `9:1`
    C
    `70%`
    D
    `80%`

    • Similar Questions

    Explore conceptually related problems

    Naturally occurring boron contain of two isotopes, whose atomic masses are 10.01 and 11.01. the atomic mass of natural boron is 10.81. calculate the percentage of each isotope in natural boron.

    Boron has two isotopes, B-10 and B-11. The average atomic mass of boron is found to be 10.80u. Calculate the percentage of abundance of these isotopes.

    The atomic mass of natural boron is 10.811. It consists of two isotopes with masses of 10.013 and 11.009. Find their fractions.

    Nitrogen occurs in nature in the form of two isotopes with atomic mass 14 and 15 respectively. If average atomic mass of nitrogen is 14.0067, what is the % abundabce of the two isotopes ?

    In nature, ratio of isotopes Boron, ""_5B^(10) and ""_5B^(11) , is (given that atomic weight of boron is 10.81)

    Home
    Profile