Problem

Phosphorus- 32 is used in the form of $\mathrm{Na…

00:55

Problem 32 Medium Difficulty

Iodine-131 is used to treat thyroid cancer.
(a) The isotope decays by $\beta$ particle emission. Write a balanced equation for this process.
(b) Iodine-131 has a half-life of 8.04 days. If you begin with $2.4 \mu \mathrm{g}$ of radioactive $^{131} \mathrm{I},$ what mass remains after 40.2 days?

Answer

a. $I_{53}^{131}->X e_{54}^{131}+e_{-1}^{0}$
b. $\frac{1}{32} \times 2.4 \mu g=0.075 \mu g$

Topics

Nuclear Chemistry

Atoms, Molecules and Ions

Book Cover for Chemistry and Chemi…

Chemistry and Chemical Reactivity 6th

Chapter 23

Nuclear Chemistry

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Top Chemistry 102 Educators

TD

Theodore D.

Carleton College

Lizabeth T.

Numerade Educator

Stephen P.

Drexel University

Allea C.

University of Maryland - University College

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Video Transcript

first will write the nuclear reaction for the decomposition of iodine 31 through beta mission producing scene on 1 31 Then we can use the half life in order to calculate the rate constant in units of one over days. Then we use the first order integrated rate law where we take the natural log of what remains over. What we start with is equal to negative. Katie plug in our negative K value. Forget time that passes 40.2 days doing a little bit of algebra. Get the natural log of X, then is equal to this expression here. So the natural log of X is negative. 2.5895 Take the anti natural log and X is going to be 0.5 point 0751 micrograms.

David C.

Weber State University

Topics

Nuclear Chemistry

Atoms, Molecules and Ions

Book Cover for Chemistry and Chemi…

Chemistry and Chemical Reactivity 6th

Chapter 23

Nuclear Chemistry

Top Chemistry 102 Educators

TD

Theodore D.

Carleton College

Lizabeth T.

Numerade Educator

Stephen P.

Drexel University

Allea C.

University of Maryland - University College