Calculate the atomic mass (average) of chlorine using the following data :

	% Natural Abundance	Molar Mass
${}^{35}Cl$	75.77	34.9689
${}^{37}Cl$	24.23	36.9659

Q.

Calculate the atomic mass (average) of chlorine using the following data:

	% Natural Abundance	Molar Mass
35Cl	75.77	34.9689
37Cl	24.23	36.9659

Q. Calculate the atomic mass (average) of chlorine using the following data:

$\begin{array}{ccc}\text{Isotopes}& \%\text{Natural Abundance}& \text{Molar mass}\\ {}^{35}\text{Cl}& 75.77& 34.9689\\ {}^{27}\text{Cl}& 24.23& 36.9659\end{array}$

Q. Natural chlorine consists of ${}^{35}$Cl and ${}^{37}$Cl . Their atomic masses are $34.97$ amu and $36.97$ amu, respectively. If the average atomic mass of chlorine is $35.5$ amu , the abundance of ${}^{35}$Cl is :

Q. Chlorine has two stable isotopes: Cl-35 and Cl-37 with atomic masses 34.96 and 36.95, respectively. If the average mass of chlorine is 35.43, calculate the percentage abundance.

Q. Natural chlorine contains chlorine in the form of the isotope ${}^{35}Cl(75.5$%) and ${}^{37}Cl$(24.5%). Calculate the average atomic mass of natural chlorine.