A 18.4 mg sample is made up of isotopically enhanced C6F14, using the same procedure described in the previous question. This chemical is used to carry oxygen to the lungs of severe burn victims, and doctors want to use the radioactive version to see if it moves from the lungs to other places in the body. Using the molar mass of fluorine that you calculated for this sample, determine how many moles of labeled fluorine are present in the sample.Express your answer in scientific notation without units. (Ex. 132.8 mg is entered as 1.328*10^2)
A 18.4 mg sample is made up of isotopically enhanced C6F14, using the same procedure described in the previous question. This chemical is used to carry oxygen to the lungs of severe burn victims, and doctors want to use the radioactive version to see if it moves from the lungs to other places in the body. Using the molar mass of fluorine that you calculated for this sample, determine how many moles of labeled fluorine are present in the sample.Express your answer in scientific notation without units. (Ex. 132.8 mg is entered as 1.328*10^2)
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter2: Atoms And Molecules
Section: Chapter Questions
Problem 2.86PAE: 2.86 For some uses, the relative abundance of isotopes must be manipulated. For example, a medical...
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2. A 18.4 mg sample is made up of isotopically enhanced C6F14, using the same procedure described in the previous question. This chemical is used to carry oxygen to the lungs of severe burn victims, and doctors want to use the radioactive version to see if it moves from the lungs to other places in the body.
Using the molar mass of fluorine that you calculated for this sample, determine how many moles of labeled fluorine are present in the sample.Express your answer in scientific notation without units. (Ex. 132.8 mg is entered as 1.328*10^2)
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