Using a deuteron beam, a sample of isotopically enriched fluorine is generated, consisting of 18F and 19F. Because this is not a natural sample, the average atomic mass on the periodic table cannot be used! Given the following abundances in the sample, calculate the new atomic mass (in amu) of the fluorine in the sample. Do not include units in your answer. Show work and upload that work to the final question of this quiz. 18F: 18.01 amu, 71.79% 19F: 19.008 amu, 28.21%
1. Using a deuteron beam, a sample of isotopically enriched fluorine is generated, consisting of 18F and 19F.
Because this is not a natural sample, the
Given the following abundances in the sample, calculate the new atomic mass (in amu) of the fluorine in the sample. Do not include units in your answer. Show work and upload that work to the final question of this quiz.
18F: 18.01 amu, 71.79%
19F: 19.008 amu, 28.21%
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)
3. Due to a (severe) labeling mistake, you find a sample of C6F14 that may or may not be labeled! Through some clever experimentation using gases, you learn that the sample contains 0.873 moles of C6F14 and has a total mass of 295.111 g. Has this sample been isotopically enhanced? How do you know?
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
