Home
Class 11
CHEMISTRY
Chlorine is a mixture of two isotopes wi...

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.

Text Solution

Verified by Experts

Average atomic mass of chlorine `= ((35 u xx 3 ) + (37 u xx 1 ))/( 3 + 1 ) = 35.5 u`
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

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 .

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.

In each of the following question, an Assertion (A) is following by a corresponding Reason (R ). Use the following keys to choose the appropriate answer. Assertion : Average atomic mass of an element depends upon the atomic masses of different isotopes and their fractional abundances. Reason : Average atomic mass is obtained by multiplying the atomic mass of the heavier isotope with its fractional abundances.

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.