Chlorine has two naturally stable isotopes: 35Cl (34.968853 amu) and 37Cl (36.965903 amu). The natural abundance of each isotope varies in different regions of the universe. In the Gribble region of space, the molar mass for a sample of chlorine is 36.36575 g/mol. Using only these three values, determine the relative percent abundance of 35Cl.

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Ansley Orozco

Chemistry

14 April, 05:23

Chlorine has two naturally stable isotopes: 35Cl (34.968853 amu) and 37Cl (36.965903 amu). The natural abundance of each isotope varies in different regions of the universe. In the Gribble region of space, the molar mass for a sample of chlorine is 36.36575 g/mol. Using only these three values, determine the relative percent abundance of 35Cl.

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Curtis Miles · Answer 1

35Cl ⇒ 34.968853 amu has an abundance of 30.05%

Explanation:

The molar mass of chlorine, (which is the average of all its naturally stable isotope masses), is 36.36575 amu.

There are 2 naturally stable isotopes, this means together they have an abundance of 100%

The isotopes are:

35Cl ⇒ 34.968853 amu has an abundance of X %

37Cl ⇒ 36.965903 amu has an abundance of Y %

X + Y = 100% OR X = 100% - Y

36.36575 = 34.968853X + 36.965903Y

36.36575 = 34.968853 (1-Y) + 36.936.96590365903Y

36.36575 = 34.968853 - 34.968853Y + 36.965903Y

1.396897 = 1.99705Y

Y = 0.699 = 69.95%

X = 100-69.9 = 30.05%

To control, we can plug in the following equation:

34.968853 * 0.3005 + 36.965903 * 0.6995 = 36.3658

This means

37Cl ⇒ 36.965903 amu has an abundance of 69.95 %

35Cl ⇒ 34.968853 amu has an abundance of 30.05%