Question

An element of average atomic weight 2Z consists of two isotopes of mass number Z and 3Z percentage of abundance of heavier isotopes.​

Answer 1

Answer:

Given,

Mass of isotope 1 = Z-1

% abundance of isotope 1 = x% =\frac{x}{100}

100

x

Mass of isotope 2 = Z+2

% abundance of isotope 2 = (100-x)%=\frac{100-x}{100}

100

100−x

Formula used for average atomic mass of an element :

\text{ Average atomic mass of an element}=\sum(\text{atomic mass of an isotopes}\times {{\text { fractional abundance}})

Z=\sum[(Z-1\times \frac{x}{100})+(Z+2\times \frac{100-x}{100})Z=∑[(Z−1×

100

x

)+(Z+2×

100

100−x

)

Solving for x, we get

x=66.66%x=66.66