The element lead (Pb) consists of four naturally occurring isotopes with masses of 203.97302, 205.97444, 206.97587, n 207.97663 amu. The relative abundances of these four isotopes are 1.4, 24.1, 22.1 and 52.4%, respectively. From this data, calculate the atomic mass of lead.

Question

Laney Stein

Chemistry

30 April, 13:59

The element lead (Pb) consists of four naturally occurring isotopes with masses of 203.97302, 205.97444, 206.97587, n 207.97663 amu. The relative abundances of these four isotopes are 1.4, 24.1, 22.1 and 52.4%, respectively. From this data, calculate the atomic mass of lead.

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Answers (1)

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Selina Harrell · Answer 1

The atomic mass of lead is: 207.216 u

Explanation:

data Isotopes mass percent

1 203.97302 1.4

2 205.974444 24.1

3 206.97587 22.1

4 207.97663 52.4

atomic mass = (203.97302x 0.014) + (205.974444 x 0.241) +

(206.97587 x 0.221) + (207.97663 x 0.524)

atomic mass = 2.856 + 49.639 + 45.742 + 108.979

atomic mass = 207.216 u