Naturally occurring B consists of two isotopes, whose atomic weights are 10.01 and 11.01. The atomic weight of natural boron is 10.81. The % of each isotope in natural boron is :
% of isotope of mass 10.01 = 20, % of isotope of mass 11.01 = 80
% of isotope of mass 10.01 = 30, % of isotope of mass 11.01 = 70
% of isotope of mass 10.01 = 50, % of isotope of mass 11.01 = 50
none of these
A
% of isotope of mass 10.01 = 20, % of isotope of mass 11.01 = 80
B
none of these
C
% of isotope of mass 10.01 = 30, % of isotope of mass 11.01 = 70
D
% of isotope of mass 10.01 = 50, % of isotope of mass 11.01 = 50
Open in App
Solution
Verified by Toppr
Average atomic weight =relative atomic mass of type 1 X % abundance of type 1+relative mass of type 2 X % abundance of type 2 100
Was this answer helpful?
2
Similar Questions
Q1
Naturally occurring boron consists 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.
View Solution
Q2
Naturally occurring B consists of two isotopes whose atomic masses are 10.01 and 11.01. The atomic mass of natural boron is 10.81. What is the % of each isotope in natural boron?
View Solution
Q3
Naturally occurring B consists of two isotopes, whose atomic weights are 10.01 and 11.01. The atomic weight of natural boron is 10.81. The % of each isotope in natural boron is :
View Solution
Q4
Naturally occurring boron has two isotopes whose atomic weights are 10.01 (I) and 11.01 (II). Atomic weight of natural boron is 10.81 The percentage of isotopes (I) and (II) respectively are :
View Solution
Q5
Atomic mass of boron is 10.81 amu. It has two isotopes with 80% and 20% abundance respectively. The atomic mass of one isotope is 11, the mass of other isotope is: