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27 February, 23:05

Americium-241 is used in smoke detectors. It has a first-order rate constant for radioactive decay of k = 1.6x10^-3yr-1. By contrast, iodine-125, which is used to test for thyroid functioning, has a rate constant for radioactive decay of k = 0.011 day-1.

(a) What are the half-lives of these two isotopes?

(b) Which one decays at a faster rate?

(c) How much of a 1.00-mg sample of each isotope remains after three half-lives?

(d) How much of a 1.00-mg sample of each isotope remains after 4 days?

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  1. 28 February, 00:23
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    A. 433 years and 63 days

    B. Iodine

    C. 0.125mg

    D. 1.00mg

    Explanation:

    A. Americium

    The formula of a radioactive decay constant half life is t = 0.693/k

    Where k is the decay constant.

    For americium, k = 0.0016

    t = 0.693/0.0016 = 433.125 apprx 433 years

    For iodine, k = 0.011

    Half life = 0.693/0.011 = 63 days.

    B. Iodine decays at a faster rate.

    C. After three half lives

    For both, first half life yields a mass of 0.5mg, next yields 0.25mg, next yield 0.125mg

    D. 1.00mg still remains.

    Half life is high for both so the decay after one day is insignificant.
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