Respuesta :
w₁(¹²C)=0.9889 (98.89%)
w₂(¹³C)=0.01108 (1.108%)
A(¹²C)=12
A(¹³C)=13
A(C)=w₁A(¹²C)+w₂A(¹³C)
A(C)=0.9889*12+0.01108*13=12.01084 a.m.u.
w₂(¹³C)=0.01108 (1.108%)
A(¹²C)=12
A(¹³C)=13
A(C)=w₁A(¹²C)+w₂A(¹³C)
A(C)=0.9889*12+0.01108*13=12.01084 a.m.u.
Answer:
We will determine the weighted average of the atomic mass of two isotopes.
Explanation:
The atomic mass of an element is the weighted average of atomic masses of the most abundant isotopes occur in nature.
Given:
Percentage abundance of C-12 : 98.89%
Percentage abundance of C-13: 1.108%
The atomic mass of carbon will be"
[tex]atomicmass=\frac{percentageofC12Xatomicmass+percentageofC13Xatomicmass}{100}[/tex]
Atomic mass = [tex]\frac{98.89X12+1.108X13}{100}=12.101[/tex]g/mol