9. A sample of a compound is found to have a half-life of 14.65 seconds. Answer the following questions regarding this sample. For your calculations, use the value of k that you found in step 4a. k= 1.22 x 10^4 a How long would it take for the sample to decompose to where 60.5% of the original sample remains? Show your calculation. b. How long would it take for the sample to decompose to where 35.896 of the original sample remains? Show your calculation.
9. A sample of a compound is found to have a half-life of 14.65 seconds. Answer the following questions regarding this sample. For your calculations, use the value of k that you found in step 4a. k= 1.22 x 10^4 a How long would it take for the sample to decompose to where 60.5% of the original sample remains? Show your calculation. b. How long would it take for the sample to decompose to where 35.896 of the original sample remains? Show your calculation.
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Chapter18: The Nucleus: A Chemist's View
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Transcribed Image Text:9. A sample of a compound is found to have a half-life of 14.65 seconds, Answer the
following questions regarding this sample. For your calculations, use the value of k that
you found in step 4a.
k%3D1.22 x 10^-4
a How long would it take for the sample to decompose to where 60.5% of the
original sample remains? Show your calculation.
b. How long would it take for the sample to decompose to where 35.8% of the
original sample remains? Show your calculation.
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This question is related to chemical kinetics.
A first-order reaction is a chemical reaction in which the rate is linearly dependent on the concentration of only one reactant.
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