**Mass Spectrometry and Isotopic Analysis****Problem Statement:**A pure sample of an element was vaporized and injected into a mass spectrometer, and the data was plotted on the graph shown. The mass values for the isotopes were found to be: - A-24: 23.985 amu- A-25: 24.986 amu- A-26: 25.983 amuFind the average atomic mass and identify the element.**Graph Explanation:**The graph displays the percent abundance of each isotope of the element along the y-axis, which ranges from 0 to 90 percent. The x-axis represents the mass number of the isotopes:- Isotope A-24 has a percent abundance of 78.99%.- Isotope A-25 has a percent abundance of 10.00%.- Isotope A-26 has a percent abundance of 11.01%.**Instructions:**To calculate the average atomic mass, multiply the mass of each isotope by its relative abundance (expressed as a decimal), and then sum these values.**Calculation Steps:**1. Convert percentages to decimals: - A-24: 0.7899 - A-25: 0.1000 - A-26: 0.11012. Calculate the contributions of each isotope to the average atomic mass: - Contribution of A-24: \(23.985 \, \text{amu} \times 0.7899\) - Contribution of A-25: \(24.986 \, \text{amu} \times 0.1000\) - Contribution of A-26: \(25.983 \, \text{amu} \times 0.1101\)3. Sum the contributions to find the average atomic mass.4. Use the resulting average atomic mass to identify the element.Finally, ensure to show all work as instructed in the note beside the graph.**Note:**- Proper documentation and calculation are essential for identifying the element based on the given isotopic data.

Answered: Image /qna-images/answer/30e42f35-9781-480c-a34b-1a0603e6f2e7.jpg

8) A pure sample of an element was vaporized and injected into a mass spectrometer and the data was plotted on the graph below. The mass values for the isotopes were found to be: A-24 (23.985 amu), A-25 (24.986 amu), and A-26 (25.983). Find the average atomic mass and identify the element. 78.99 Percent Abundance 90 SO 70 60 50 40 30 20 10 0- gr 24 10.00 11.01 26 25 Mass Number 0.00 27 Show proper work!

8) A pure sample of an element was vaporized and injected into a mass spectrometer and the data was plotted on the graph below. The mass values for the isotopes were found to be: A-24 (23.985 amu), A-25 (24.986 amu), and A-26 (25.983). Find the average atomic mass and identify the element. 78.99 Percent Abundance 90 SO 70 60 50 40 30 20 10 0- gr 24 10.00 11.01 26 25 Mass Number 0.00 27 Show proper work!

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Lithium, is used in dry cells and storage batteries and in high temperatures lubricants, it has two naturally occurring isotopes, 6Li and 7Li. Calculate the atomic mass of lithium. isotopic mass(amu): 6.015217.016003 abundance(%): 7.50 92.50
Consider the following data for the hypothetical element Smileonium, So. What is the average atomic mass of Smileonium? Isotope Relative Atomic mass So-46 46.046 u So-51 50.826 u 48.44 u 48.50 u 49.11 u 47.76 u 47.44 u Percent Abundance 64.08% 35.92%
How many neutrons are in 37.0 ug ( ug= 10^-6 g) of 14 6 C? You may assume that the atomic mass of 14 6 C is exactly 14.0 U. Avogadro's number = 6.022 x10^23
A hypothetical element, M, with average atomic weight of 35.75. M has three stable isotopes with the masses and percentage abundances are shown below. Identify missing information on the table. Isotopes Mass (amu) Abundance 34M 33.99 46.78 37M ? 33.93 38M 37.96 ? 3/M mass = 36.87 amu, 38M percentage abundance = 19.64%. 37 'M mass = 36.29 amu, 38M percentage abundance = 19.89%. %3D 3/M mass = 36.92 amu, 38M percentage abundance = 19.29%. 37M mass = 36.92 amu, 38M percentage abundance = 20.29%. %3D %3D 37 'M mass = 32.92 amu, 3ºM percentage abundance = 19.29%.
The element zirconium has five naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. Show your work to determine the average atomic mass. Isotope Mass % Abundance Zr-90 89.9043 51.40 Zr-91 90.9053 11.20 Zr-92 91.9046 17.10 Zr-94 93.9061 17.50 Zr-96 95.9082 2.80
An element has three naturally occurring isotopes with the following masses and abundances: Isotopic Fractional Mass Abundance (ати) 19.992 0.9048 20.994 0.0027 21.991 0.0925 Calculate the atomic weight of this element. What is the identity of the element? Atomic weight amu Element is
Using the following data, determine the percent abundance of the third isotope and the average atomic mass of isotope X. Give as a percentage. X-22 atomic mass = 22.10498 abundance = 52.3985% X-23 atomic mass = 23.0005 abundance = 24.8731% X-24 Atomic mass = 24.0593
Element A has two isotopes. The first isotope is present 19.41% of the time and has a mass of 231.12. The second isotope has a mass of 193.24. Calculate the atomic mass of element A.
Naturally occurring neon exists as three isotopes. 90.51% is Ne-20 with a mass of 19.99 amu, O.27% is Ne-21 with a mass of 20.99 amu, and9.22% is Ne-22 with a mass of 21.99 amu. What is the atomic mass of neon? O 20.18 amu O 62.97 amu O 10.00 amu O 20.99 amu
A hypothetical element exists as two isotopes: I = 68.00 amu and II = 71.00 amu. If the percent abundance of isotope I is (6.61x10^1)%, what would be the calculated atomic mass (in amu)?
A certain element has five stable isotopes with the following masses and percent abundance: Isotope 1: 63.929147 amu, 48.63% Isotope 2: 65.926037 amu, 27.90% Isotope 3: 66.927131 amu, 4.100% Isotope 4: 67.924848 amu, 18.75% Isotope 5: 69.925325 amu, 0.6200% What is the atomic mass of this element? (Do not round intermediate calculations.)
6) Complete the following table by calculating the atomic mass. Isotope Mass of Atom (u) Percent Abundance (%) ¹H 2H 12C 13C 160 170 180 1.007825 2.1040 12.0 13.003355 15.994915 16.999131 17.999160 99.985 0.015 98.90 1.10 99.762 0.038 0.200 Atomic Mass (u)