It can be shown using mass spectrometry that the ratio of naturally occurring chlorine -35 to its isotope chlorine -37 is 3 : 1. Assuming that no other isotopes existed, what would be the atomic weight of chlorine?

35.5

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37.5

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36.6

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None of the above

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Solution

The correct option is A $35.5$
Atomic weight of chlorine= $\frac{3 \times 35 + 1 \times 37}{4} = 35.5$

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Similar questions

Naturally occurring chlorine consists of two isotopes whose atomic weights are 35 and 37. The atomic weight of natural chlorine is 35.5, then what is the ratio of $C l^{35} t o C l^{37}$ ?

Q. Chlorine has two naturally occuring isotopes

_{17}^{37} C l

and

_{17}^{35} C l

and average atomic mass of chlorine is

35.5

. The percentage of

_{17}^{37} C l

is:

Q. Atomic mass of chlorine is 35.5. It has two isotopes of atomic mass 35 and 37. The percentage of heavier isotope is:

Q. Chlorine exists in two isotopic forms,

C l - 37

and

C l - 35

but its atomic mass is

35.5

. This indicates the ratio of

C l - 37

and

C l - 35

is approximately:

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It can be shown using mass spectrometry that the ratio of naturally occurring chlorine -35 to its isotope chlorine -37 is 3 : 1. Assuming that no other isotopes existed, what would be the atomic weight of chlorine?

The correct option is A 35.5Atomic weight of chlorine=3×35+1×374=35.5

The correct option is A $35.5$
Atomic weight of chlorine= $\frac{3 \times 35 + 1 \times 37}{4} = 35.5$